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1. Consider the reaction: 2HgO(s) ⇄ 2Hg(l) + O2(g)
which of following will shift the equilibrium toward the reactants? I) more solid HgO is added;
II) decreasing the pressure;
III) more O2 is added
- I and III
- II only
- I, II and III
- III only
NO2(g) + CO(g) ⇄
2. Consider the reaction:
A 1L vessel at 400C contains the equilibrium concentrations [NO] = 0.1 M, [CO2]= 0.02 M, [NO2] = 0.01 M, and [CO] = 0.1M. What is the value of the equilibrium constant Kc for the reaction?
a. 0.5
b. 5
c. 1
d. 2
A 1L vessel at 400C contains the equilibrium concentrations [NO] = 0.1 M, [CO2]= 0.02 M, [NO2] = 0.01 M, and [CO] = 0.1M. What is the value of the equilibrium constant Kc for the reaction?
a. 0.5
b. 5
c. 1
d. 2
3. Determine the pH of a 5.5 ×10−2M solution of H2SO4.
a. 1.25
b. 0.95
c. 7.00
d. 6.48
4. Which of the following mixtures can produce a buffer?
- CH3COOH, CH3COONa
- H++OH−
- HCl + NaOH
- all of the above
- increased by 3 M
- decreased by 3 M
- increased by a factor of 1000
- decreased by a factor of 100
6. If the pH of HNO3 solution is 2.45, what is the molarity of this solution?
a. F-
a. 4.00
b. 10.00
c. 6.00
- 3.5 × 10−3M
- 2.45 × 10−5 M
- 2.81×102M
- Can’t be calculated
a. F-
- H2O+
- H3O
- Can’t be determined
- basic
- acidic
- neutral
- None of the above
- Nitrous acid
- Acetic acid
- Sulfuric acid
- water
a. 4.00
b. 10.00
c. 6.00
d. 7.00
14. A solution with [H+] = 5 x10-11 M would have a pH ------and would be considered -------
the endpoint. What is the concentration of the KOH? a) 0.115 M
b) 0.230 M
c) 0.169 M
d) 0.0848 M
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- between 1 and 2; acidic
- between 10 and 11; basic
- 2; basic
- 2; acidic
the endpoint. What is the concentration of the KOH? a) 0.115 M
b) 0.230 M
c) 0.169 M
d) 0.0848 M
If you have any test reviews, homeworks, guides, anything school related that you think can be posted on this website, reach out to me at makingschooleasier@gmail.com