General Chemistry 1

2 Na + Cl$_2$ $\longrightarrow$ 2 NaCl

How many grams of Cl$_2$ are needed to react completely with 12.0 g of Na?

The theoretical yield for a reaction is 627.0 g of SF$_6$. An experiment only yields 627.8g. What is the percent yield?

4 H$_2$ (g) + CS$_2$ (g) $\longrightarrow$ CH$_4$ + 2 H$_2$S (g)

Methane and hydrogen sulfide form when hydrogen reacts with carbon disulfide. Identify the excess reagent and calculate the remaining mass after 36 L of H$_2$ reacts with 12 L of CS$_2$

Many metals react with oxygen gas to form the metal oxide. When solid calcium and oxygen gas react they form a metal oxide. You wish to calculate the mass of metal oxide that can be prepared from 4.20 g of Ca and 2.80 g of O$_2$

A. Predict the metal oxide product formed when solid calcium and oxygen gas react (include states of matter.) Balance the equation.

B. How many moles of product can be produced from the given mass of Ca?

C. How many moles of product can be produced from the given mass of O$_2$ ?

D. What is the limiting reactant?

Zn + 2HCl $\longrightarrow$ ZnCl$_2$ + H$_2$

How many grams of Zn will react with 25.0 mL of 3.0 M HCl?

How many grams of AgNO$_3$ are needed to prepare 250 mL of 0.0125 M AgNO$_3$? (MM of AgNO$_3$ = 169.87 g/mol)

How could 100 mL of 0.125 M H$_2$SO$_4$ solution be made from 0.500 M H$_2$SO$_4$ solution?

How many milliliters of 0.124 M NaOH contain enough NaOH to react with 15.4 mL of 0.108 M H$_2$SO$_4$ ?

2 NaOH + H$_2$SO$_4$ $\longrightarrow$ 2 H$_2$O + Na$_2$SO$_4$

How many moles of BaSO$_4$ will form if 20.0 mL of 0.600 M BaCl$_2$ is mixed with 30.0 mL of 0.500 M MgSO$_4$?

BaCl$_2$ + MgSO$_4$ $\longrightarrow$ BaSO$_4$ + MgCl$_2$

Write the complete, ionic, and net ionic equations for the reaction of CH$_3$NH$_2$ with HC$_2$H$_3$O$_2$ .

5 SO$_2$ + MnO$_4^-$ + 2 H$_2$O $\longrightarrow$ 5 SO$_4^{2-}$ + 2 Mn$^{2+}$ + 4 H$^+$

Assign oxidation numbers for each of the atoms in the above net ionic equation. Identify the oxidizing and reducing agents.

The density of sea water is 1.03 g/mL. What mass of seawater would fill a vessel to a volume of 255 mL?

How many liters of hydrogen, measured at STP, are needed to combine exactly with 1.50 L of nitrogen, also at STP, to form ammonia?

n$_2$ + 3 H$_2$ $\longrightarrow$ 2 NH$_3$

The label on a cylinder of a noble gas became illegible, so a student allowed some of the gas to flow into a gas bulb with a volume of 0.3000 L until the pressure was 0.901 atm. The sample then weighed 1.45 g and its temperature was 27.0 $^{\circ}$C. What is the molar mass of the gas? Which noble gas is it?

One procedure used to separate the isotopes of uranium to obtain material to construct a nuclear weapon employs uranium compound with the formula UF$_6$ . The compound boils at about 56 $^{\circ}$C, so at 100 $^{\circ}$C it is a gas. What is the density of 1.00 mol of UF$_6$ at 100 $^{\circ}$C if the pressure of the gas is 0.974 atm. (MM of U = 352.0 g/mol)

A sample of gas has a pressure of 1.5 atm and a volume of 500.0 mL. What would be the pressure if the volume were compressed to 325.0 mL at a constant temperature?

Find the molar mass of 15.0 g of a gas in a 2.0 L container at 291 K and 1.3 atm.

Calculate the density (g/L) of methane ( CH$_4$ ) at 1.0 atm and 278 K.

Mg(s) + 2 HCl(aq) $\longrightarrow$ MgCl$_2$(aq) + H$_2$(g)

50.0 mL of 3.0 M HCl reacts with excess Mg in a closed 4.0 L container at 295 K. What is the pressure from the hydrogen gas that is produced?

A sample of oxygen is collected over water at 20 $^\circ$C and a pressure of 738 torr. What is the partial pressure of oxygen in mmHg??