When 3.00 g of NH3(g) (M = 17.03 g/mol) reacts with 18.0 g of HCl(g) (M = 36.46 g/mol), what is the theoretical yield of NH4Cl(s) in grams?

What volume, in liters, of carbon monoxide gas at 78.5 °C and 848 torr is needed to produce 4.54 g of methanol, CH₃OH, according to the reaction: CO(g) + 2 H₂(g) → CH₃OH(g)?

What volume, in liters, of hydrogen gas at 32.5 °C and 722 torr is needed to produce 0.224 g of methanol, CH₃OH, according to the reaction: CO(g) + 2 H₂(g) → CH₃OH(g)?

What volume, in liters, of sulfur dioxide gas at 455 K and 2.03 atm is needed to produce 89.6 g of sulfur trioxide, SO₃, according to the reaction: 2 SO₂(g) + O₂(g) → 2 SO₃(g)?

What volume, in mL, of 1.34 M RbOH(aq) is needed to completely neutralize 146 mL of 1.56 M H2SO4(aq)?

When 100.0 mL of 0.100 M AgNO3 solution is mixed with 200.0 mL of 0.100 M NaBr solution in a coffee cup calorimeter, the temperature of the mixed solution rises from 23.48°C to 24.16°C. Ignore the heat absorbed by the calorimeter. Determine the limiting reactant.

When 50.0 mL of 0.104 M HClO4 and 75.0 mL of 0.0753 M NaOH are combined, 291 J of heat are produced. If the initial temperature of both solutions was 22.5°C, determine the final temperature of the solution. Assume the density of the solution is 1.00 g/mL and the specific heat capacity is 4.18 J/g°C.

When methane (CH4) burns, it reacts with oxygen gas to produce carbon dioxide and water. The unbalanced equation for this reaction is CH4(g) + O2(g) → CO2(g) + H2O(g). This type of reaction is referred to as a complete combustion reaction. What mass of carbon dioxide (CO2) is produced when 16 grams of methane is completely combusted?

Which answer choice shows the correct ratio of moles Ni:PO4^3- for the reaction of aqueous NiCl2 with Na3PO4?