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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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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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Solid arsenic reacts with Oxygen gas to synthesize solid arsenic trioxide. How many moles of arsenic trioxide will be produced from 3.4 moles of oxygen gas?
$4As$ + $ 3O_2$ -----> $2As_2O_3$ According to equation $3$ moles of oxygen gas is required to form arsenic trioxide = $2$ moles $3.4$ moles of O2 will be required...
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Water, H2O, is made via its formation reaction. How many moles of water form when (7.69x10^0) moles of oxygen gas react? (Answer in mol to 3 s.d. in proper scientific notation)
Start with a balanced equation. It will be used to determine mol ratios between the product and the reactant. $"2H"_2 + "O"_2$$rarr$$"2H"_2"O"$ Multiply the given mol oxygen gas by the...
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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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How many moles of water are produced when $"2.15 moles"$ of oxygen gas react with excess hydrogen gas?
$"I mol"$ of $"O"_2$ produces $"2 moles"$ of $"H"_2"O"$, so $"2.15 moles"$ of $"O"_2$ produce $2/1×2.15 = "4.30 moles H"_2"O"$
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Propane, $C_3H_8$, reacts with oxygen to produce carbon dioxide and water. If 10.0 grams of oxygen reacts with an excess of propane, then how many moles of carbon dioxide were produced?
Given: Mass of $"O"_2$; chemical equation (understood) Find: Moles of $"CO"_2$ Strategy: The central part of any problem is to convert moles of something to moles of something else....
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If iron (II) oxide gas decomposes into iron liquid and oxygen gas and 6 moles of iron (II) oxide gas are used, how of liters of oxygen gas are produced?
This means that for $6mol$ of $FeO$, only $3mol O_2$ is produced (half the moles). The volume of the oxygen is dependant on temperature and pressure. E.g. : If...
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How can I solve this ??
dentify the electrolyte solution with the largest concentration of ions.
A. 1.0 moles KOH in 2.0 L water
B. 1.0 moles AlCl3 in 2.0 L water
C. 1.3 moles MgCl2 in 3.0 L water
D. 1.5 moles NaCl in 4.0 L water
will generally dissociate into ions in solution. For the purposes of this problem, let's assume there isn't much ion pairing. The key here is knowing we're worried about...
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What is the oxidation number of oxygen in $"sodium peroxide"$, $Na_2O_2$?
When we assign , we assign conceptual charges to the individual atoms such that when these charges are summed up we get the charge on the molecule or the ion....
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