5 Glaring Signs Your Coworkers Are Untrustworthy

5 Glaring Signs Your Coworkers Are Untrustworthy You don’t have to be best friends with your coworkers. We know some of you want to keep the personal and the professional separate, and that’s totally fine. But at the very least, you should be able to trust your coworkers. You certainly wouldn’t want to find out that someone else in the office has been taking credit for your hard work or passing along things you say in confidence to the wrong people. So it is wise to take note of when a colleague may be less than honest. Here are 5 signs that will help you weed out the untrustworthy.1. You’re the subject of gossip.Have you ever suspected that a coworker was whispering behind your back? And do you suspect that the coworker is whispering about you? Are things you said to that coworker in private getting around the office? These are all warning signs that someone is gossiping about you. And you can never trust a gossip.2. You’ve been robbed.Did you ever have a great idea that you mentioned to a cowork er who then went ahead and passed off that idea as his or her own? That’s not so much a warning sign as a great big flashing red light alerting you that he or she is not honest. It would be ideal to work in an environment in which having your ideas or work stolen is not a concern, but sometimes it’s best to keep your best ideas close to your chest.If this does happen to you, don’t be shy about having a private meeting with your manager to talk about the issue and how you should handle it in the future.3. You’re being left out.Ever find yourself left out of important meetings or email threads? Maybe these are just a harmless oversights, but finding yourself chronically left out might indicate that a coworker is jealous of your abilities and does not want you to shine by participating in crucial office confabs. If you find that it’s always the same coworker who is â€Å"accidentally† leaving you out of those meetings of minds, that coworker mi ght have an axe to grind against you. Again, please don’t feel out of line by reporting this type of behavior should be reported to management.4. You’re the scapegoat.Do you sometimes get blamed for mistakes you didn’t make? Do you feel fingers pointing at you behind your back? Then someone might be trying to turn you into the office scapegoat. This may be random harassment, or someone might be trying to cover up her or his own blunders by making them yours. If you regularly find yourself taking the heat for someone else’s screw-ups, that someone might be the culprit behind your scapegoat status.Always stand up for yourself and  get everything in writing. Even if you have to shoot off a quick â€Å"just confirming what we discussed at my desk this afternoon† email, do it. You can never be too safe.5. You’re the victim of sabotage.Did a project you worked hard on end up getting lost or a well-organized presentation end up mysteriously turni ng into a mess? Then someone might be deliberately sabotaging your work. Yes, it seems juvenile, but these things do happen in the adult work world. Just be sure that there is strong evidence that a particular coworker is sabotaging your work before making any accusations. You don’t want to falsely accuse anyone or mistakenly blame a coworker for your own errors. Then your coworkers might start thinking that you’re the one who isn’t completely trustworthy.

Calculating the Change in Entropy From Heat of Reaction

Calculating the Change in Entropy From Heat of Reaction The term entropy refers to disorder or chaos in a system. The greater the entropy, the greater the disorder. Entropy exists in physics and chemistry, but can also be said to exist in human organizations or situations. In general, systems tend toward greater entropy; in fact, according to the second law of thermodynamics, the  entropy  of an isolated system can never spontaneously decrease. This example problem demonstrates how to calculate the change in entropy of a systems surroundings following a chemical reaction at constant temperature and pressure. What Change in Entropy Means First, notice you never calculate entropy, S, but rather change in entropy,  ÃŽâ€S. This is a measure of the disorder or randomness in a system. When  ÃŽâ€S is positive it means the surroundings increased entropy. The reaction was exothermic or exergonic (assuming energy can be released in forms besides heat). When heat is released, the energy increases the motion of atoms and molecules, leading to increased disorder. When ΔS is negative it means entropy of the surroundings were reduced or that the surroundings gained order. A negative change in entropy draws heat (endothermic) or energy (endergonic) from the surroundings, which reduces the randomness or chaos. An important point to keep in mind is that the values for  ÃŽâ€S are for  the surroundings! Its a matter of point of view. If you change liquid water into water vapor, entropy increases for the water, even though it decreases for the surroundings. Its even more confusing if you consider a combustion reaction. On the one hand, it seems breaking a fuel into its components would increase disorder, yet the reaction also includes oxygen, which forms other molecules. Entropy Example Calculate the entropy of the surroundings for the following two reactions.a.) C2H8(g) 5 O2(g) → 3 CO2(g) 4H2O(g)ΔH -2045 kJb.) H2O(l) → H2O(g)ΔH 44 kJSolutionThe change in entropy of the surroundings after a chemical reaction at constant pressure and temperature can be expressed by the formulaΔSsurr -ΔH/TwhereΔSsurr is the change in entropy of the surroundings-ΔH is heat of reactionT Absolute Temperature in KelvinReaction aΔSsurr -ΔH/TΔSsurr -(-2045 kJ)/(25 273)**Remember to convert  °C to K**ΔSsurr 2045 kJ/298 KΔSsurr 6.86 kJ/K or 6860 J/KNote the increase in the surrounding entropy since the reaction was exothermic.  An exothermic reaction is indicated by a positive  ÃŽâ€S  value. This means heat was released to the surroundings or that the environment gained energy. This reaction is an example of a combustion reaction. If you recognize this reaction type, you should always expect an exothermic reaction a nd positive change in entropy.Reaction bΔSsurr -ΔH/TΔSsurr -(44 kJ)/298 KΔSsurr -0.15 kJ/K or -150 J/KThis reaction needed energy from the surroundings to proceed and reduced the entropy of the surroundings. A negative  ÃŽâ€S  value indicates an endothermic reaction occurred, which absorbed heat from the surroundings.Answer:The change in entropy of the surroundings of reaction 1 and 2 was 6860 J/K and -150 J/K respectively.