50 cm3 of a gaseous hydride of phosphorus, PHn reacts with exactly 150 cm3      of chlorine, Cl2 to form liquid phosphorus trichloride and 150 cm3 of    hydrogen chloride gas, HCl.    Deduce the formula of the phosphorus hydride.

Grease fires can be extinguished by applying baking soda (sodium hydrogen carbonate), which decomposes due to the heat to produce sodium oxide, carbon dioxide and water. The carbon diocide produced helps to smother the flames. How many grams of baking soda would need to be thrown on to a fire to produce 0.500 moles (approximately 11 L) of carbon dioxide gas?

For the reaction N, + 3H, 2NH, what is the Mole ratio of nitrogen to hydrogen? t. Mole ratio of hydrogen to ammonia?

See the example in Introduction for set-up of calculations. Calculate the number of a) moles of F b) atoms of F in 32.5 g of fluorine gas, F 2 .

In a lab experiment, 7.97 g of phosphorus reacts with bromine to form 69.65 g of phosphorus tribromide. (a) Calculate the percentage by mass of P in phosphorus tribromide.

A)Write the correct formula of copper (II) sulfate pentahydrate.  (b) Calculate the theoretical percentage of water in Manganese (II) sulfate heptahydrate to four significant figures. You must show all calculations clearly to get full credit.

2a. Calculate the volumes of ammonia and oxygen required to produce 28 moles of nitrogen dioxide. 4NH3(g)+7O2(g)→4NO2(g)+6H2O(l) 2b. What is the mass of nitrogen dioxide produced if the yield is 88%?

00 S Nazza .01608 ·018302 3. (part a). You are given 0.104 g of a sample of KwFex(C₂O4)y(H₂O)z. In the laboratory, you titrate this sample with 0.00940 M KMnO4 and you need 10.1 mL of the KMnO4 solution to reach the stoichiometric point. Calculate the mass and moles of [C₂04]²- in the sample. Please show all of your detailed calculations.

A 235.2-g sample of ground water is analyzed for calcium. The Ca2+ in the sample is first precipitated and filtered-off as NH4CaPO4·7H2O. This precipitate is dried and heated, releasing water and ammonia to yield anhydrous calcium pyrophosphate (Ca2P2O7). The mass of Ca2P2O7 obtained is 0.0234 g.Give the calcium content of the ground water in parts per million (to three significant figures).

A 290.3-g sample of ground water is analyzed for calcium. The Ca2+ in the sample is first precipitated and filtered-off as NH4CaPO4·7H2O. This precipitate is dried and heated, releasing water and ammonia to yield anhydrous calcium pyrophosphate (Ca2P2O7). The mass of Ca2P2O7 obtained is 0.0534 g.Give the calcium content of the ground water in parts per million