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18 Dec 2019

How many grams of calcium are consumed when 160.6 mL of oxygen gas, measured at STP, reacts with calcium according to the following reaction? 2Ca(s)+O2(g)→2CaO(s)

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Trinidad Tremblay
Trinidad TremblayLv2
31 Dec 2019

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Related questions

Question

How many grams of calcium oxide can be prepared from (7.60x10^0) grams of calcium and 3.85 grams of oxygen gas?

2Ca (s) + O2 (g) --> CaO (s)

Question

If you were only able to produce 5.25 grams of CaO in the lab , What was your percent yield.

(1) Chapter 12 Question 2 - Algorithmic

Part A

How many kJ of heat are needed to completely vaporize 43.2 g of H2O? The heat of vaporization for water at the boiling point is 40.6 kJ/mole.

How many kJ of heat are needed to completely vaporize 43.2 g of H2O? The heat of vaporization for water at the boiling point is 40.6 kJ/mole.

a. 97.4
b. 2.26
c.16.9
d. 43.2
e. none of the above

(2) Chapter 12 Question 3 - Algorithmic

Part A

A 250 gram sample of water at the boiling point had 24.0 kJ of heat added. How many grams of water were vaporized? Heat of vaporization for water is 40.6 kJ/mole.

A 250 gram sample of water at the boiling point had 24.0 kJ of heat added. How many grams of water were vaporized? Heat of vaporization for water is 40.6 kJ/mole.

a. 20.5
b. 0.591
c. 1.69
d. 10.6
e. none of the above

(3)

Chapter 12 Question 21 - True/False

Part A

Water has a heat of vaporization of 44.0 kJ/mol while the chemical diethyl ether has a heat of vaporization of 27.1 kJ/mol. This shows that one mole of water would vaporize more easily than would one mole of diethyl ether.

Water has a heat of vaporization of 44.0 kJ/mol while the chemical diethyl ether has a heat of vaporization of 27.1 kJ/mol. This shows that one mole of water would vaporize more easily than would one mole of diethyl ether.

True
False

(4)

Exercise 11.97

Part A

How many grams of calcium are consumed when 160.4 mL of oxygen gas, measured at STP, reacts with calcium according to the following reaction?
2Ca(s)+O2(g)→2CaO(s)
mCa = ???????? g

(5)

Exercise 11.79

A gas mixture contains 74% nitrogen and 26% oxygen.

Part A

If the total pressure is 1.18 atm what are the partial pressures of each component?

Express your answers using TWO significant figures. Enter your answers numerically separated by a comma.
PN2, PO2 = ?????? atm

For the reaction, calculate how many moles of the product form when 0.046 mol of O2 completely reacts.
Assume that there is more than enough of the other reactant.
2Ca(s)+O2(g)→2CaO(s)

For the reaction, calculate how many moles of the product form when 0.018 mol of O2 completely reacts.
Assume that there is more than enough of the other reactant.
4Fe(s)+3O2(g)→2Fe2O3(s)

For the reaction, calculate how many moles of the product form when 0.044 mol of K completely reacts.
Assume that there is more than enough of the other reactant.
4K(s)+O2(g)→2K2O(s)

For the reaction, calculate how many moles of the product form when 0.036 mol of O2 completely reacts.
Assume that there is more than enough of the other reactant.
4Al(s)+3O2(g)→2Al2O3(s)

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