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In a lab 178.8g of water is separated into hydrogen gas and oxygen gas. The hydrogen gas has a mass of 20.0g. What is the mass of the oxygen gas produced?
Of course, we could do this analytically, and write the chemical equation for water decomposition, and then apportion molar quantities: $H_2O(l) rarr H_2(g) + 1/2O_2(g)$, but why should I bother?...
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Oxygen and hydrogen react explosively to form water. In one reaction, 6 g of hydrogen combines with oxygen to form 54 g of water. How much oxygen was used?
I'll show you two approaches to solving this problem, one really short and one relatively long. $color(white)(.)$ SHORT VERSION The problem tells you that $"6 g"$ of hydrogen gas,...
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Using the following reaction, if 1.75 moles of nitrogen gas are reacted with excess hydrogen gas, how many moles of $NH_3$ will be produced? $N_2 + 3H_2 -> 2NH_3$?
Simply write out ratio of the known and unknown components: $(n(NH_3))/(n(N_2))=2/1$ $n(NH_3)=2n(N_2)=2xx1.75mol=3.5mol$
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In the combustion of hydrogen gas, hydrogen reacts with oxygen from the air to form water vapor. Hydrogen + Oxygen $->$ water. If you burn 58.1 g of hydrogen and produce 519 g of water how much oxygen reacted?
The stoichiometrically balanced equation tells us unequivocally that $1$ $mol$ dihydrogen reacts with $0.50$ $mol$ dioxygen to give $1$ $mol$ water. $"Moles of dihydrogen"$ $=$ $(58.1*g)/(2.02*g*mol)$ $=$ $28.7*mol$ $H_2$ $"Moles...
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Hydrogen and oxygen react chemically to form water. How much water would form if 4.8 grams of hydrogen reacted with 38.4 grams of oxygen?
We need a stoichiometric equation for water synthesis: $H_2(g) + 1/2O_2(g) rarr H_2O(l)$ Clearly, dihydrogen must be present in a 2:1 molar ratio with respect to dioxygen. $"Moles of dihydrogen"$...
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Aluminum will react with sulfuric acid in the following reaction: $2Al(s) + 3H_2SO_4(l) -> Al_2(SO_4)_3(aq) + 3H_2(g)$. How many moles of $H_2SO_4$ will react with 18 mol Al? How many moles of each product will be produced?
With reference to the given balanced equation for the , the needed number of moles for each remaining compound involved in the reaction using the mass of $Al$ as basis...
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When propane $C_3H_8$ reacts with oxygen, carbon dioxide and water are produced. If 7.51 grams of propane react with excess oxygen, how many grams of carbon dioxide are formed?
From the equation above, 3 moles of carbon dioxide result from every mole of propane combusted. We had, $(7.51*g)/(44.1*g*mol^-1)$ $=$ $?? "moles of propane"$. So how many moles of...
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Under certain conditions of temperature and pressure, hydrogen gas and nitrogen gas react to form ammonia gas. Determine the mass of ammonia produced if 3.50 moles of hydrogen has reacts with 5.00 moles of nitrogen gas?
Start by balancing the equation for the reaction between hydrogen $"H"_2$ and nitrogen $"N"_2$, which produces ammonia $"NH"_3$: $color(darkgreen)(1) color(white)(.) "N"_2 (g) + color(darkgreen)(3) color(white)(.) "H"_2 to color(darkgreen)(2) color(white)(.) "NH"_3...
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Aluminum reacts with aqueous $HBr$ to produce hydrogen gas and aluminum bromide. How many mL of hydrogen gas are produced at 1.03 atm and 20.00 $"^o$C when 0.498 g of aluminum react with an excess of $HBr$?
Each equiv of metal reduces $3$ equiv of acid, and $3/2$ equiv of dihydrogen gas are evolved. $"Moles of aluminum"$ $=$ $(0.498*g)/(26.98*g*mol^-1)=0.0185*mol$. Now, given the conditions, clearly the metal is...
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Ammonia reacts with oxygen according to the equation given below.
If a $"72.0-mL"$ sample of $"NH"_3$ gas is allowed to react with excess oxygen at room temperature, $25^@"C"$, and $"1 atm"$, calculate the number of molecules of water produced?
The first thing that you need to do here is to use the equation $color(blue)(ul(color(black)(PV = nRT)))$ Here $P$ is the pressure of the...
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