Answer: The approximate pressure of the gas after it is heated to 278 K is 0.468 atm.
Explanation:
Given: 
= 178 K, 
= 0.3 atm
= 278 K, 
= ?
According to Gay Lussac law, at constant volume the pressure of a gas is directly proportional to the temperature.
Formula used to calculate the pressure is as follows.
Substitute the values into above formula is as follows.
Thus, we can conclude that the approximate pressure of the gas after it is heated to 278 K is 0.468 atm.
Answer:
[CH₃OH] to decrease and [CO] to increase.
Explanation:
- Since the energy appears as a product. So, the system is exothermic that releases heat.
- Increasing the temperature of the system will cause the system to be shifted to the left side to attain the equilibrium again.
<em>[CH₃OH] to decrease and [CO] to increase.</em>
<em></em>
*** 2 ***
<span>if we assume volume NaCl + volume H2O = volume H2O.. i.e.. NaCl does not effect volume </span>
<span>therefore.. the units of.. </span>
<span>.. M = moles NaCl / L solution ≈ moles NaCl / L H2O </span>
<span>.. density = grams NaCl / L solution ≈ grams NaCl / L H2O </span>
<span>again.. that is our assumption </span>
<span>so we can readily see that </span>
<span>.. M = (1 mol NaCl / ___g NaCl) x (__g NaCl / L H2O) + 0 </span>
<span>ie.. </span>
<span>.. M = (1 mol NaCl / 58.5g NaCl) x density solution + 0 </span>
<span>so.. we would expect.. </span>
<span>.. m = 0.01709 mol / g </span>
<span>.. b = 0 </span>
