A student wanted to fill a small balloon with 1.00 L of H₂(g) at SATP. The hydrogen gas is produced when aluminium metal reacts with hydrochloric acid according to the following reaction: 2 Al(s) + 6 HCl(aq) → 2 AlCl3(aq) + 3 H₂(g) What mass (in g) of aluminium metal is required to react with excess hydrochloric acid to produce 1.00 L of hydrogen gas at SATP? Express your answer with three significant digits. Do not include units! g Al(s)

Hw.10.

Assuming constant conditions, how many milliliters of chlorine gas react to yield 1.15 LL of dichlorine trioxide? Cl2(g)+O2(g)→Cl2O3(g)

What volume (L) of 0.550 M hydrochloric acid solution can be prepared from the HCl produced by the reaction of 15.0 g of NaCl with excess sulfuric acid, assuming a reaction yield of 91.2%? NaCl(s) + H,SO,1) → HCl(g) + NaHSO,(s)

The reaction between SO3 (g) and CO2 (g) is based on the chemical equation below. 2 SO3 (g) +  CO2 (g) =  CS2 (g) + 4 O2 (g) At 500 oC, we mix 0.20 mol SO3 (g) 0.25 mol CO2 (g) and 1.20 mol O2 (g) (without CS2 (g)) initially in a 1-L bottle. After the reaction reaches equilibrium, the amount of SO3 (g) becomes 0.12 mol. Determine the value of the equilibrium constant of the above reaction (with 2 significant figures).

What mass (g) of NaOH is required to make 262 ml of 0.41 M NaOH(aq) solution?

Q) Drinking water may contain several unwanted ions such as phosphate ions. In order to remove the phosphate ions from the drinking water, a solution of calcium hydroxide can be added. As a result, a solid Ca5OH(PO4)3 is formed and isolated by filtration and a hydroxide ion are also formed. The reaction for this process is below: 5 Ca(OH)2 (aq) + PO43- (aq) → Ca5OH(PO4)3 (s) + OH- (aq) a) If 3.00 mL of 0.100 M calcium hydroxide is mixed with 4.00 mL of an aqueous solution of 0.0800 M phosphate ions (PO43-). What is the mass of Ca5OH(PO4)3 that can be isolated from the reaction? b) How many moles of the excess reactant remains unreacted? c) What is the concentration of the hydroxide ions in this solution? d) What is the mass of calcium (in grams) that can be recovered?

Consider the formation of chlorine gas, from household bleach (sodium hypochlorite) and hydrochloric acid.   NaClO(aq) + 2 HCl(aq) → Cl2(g) + H2O(l) + NaCl(aq) If 13.5 ml of sodium hypochlorite (d = 1.11 g/ml) reacts with excess hydrochloric acid, what volume of chlorine gas will be collected over water at 20.0 oC?  The lab barometer reads atmospheric pressure to be 755 mm Hg and the water vapor pressure at 20.0oC is 17.5 mm Hg.   Question  options:   4.05 L   4.75 L   4.39 L   4.99 L

Paylben

A 5.80-g sample of lead nitrate, Pb(NO3)2, molar mass = 331 g/mol, is heated in an evacuated cylinder with volume of 3.25 L. The salt decomposes when heated,  according to the equation:  2Pb(NO3)2(s) => 2PbO(s) + 4NO2 (g) + O2 (g) Assuming complete decomposition, what is the cylinder after decomposition and cooling to a temperature of 250 K? Assume PbO(s) takes a negligible volume.  Enter answer without a unit.