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As for all these problems, we first need a stoichiometrically balanced equation,
And thus between the oxide and the starting metal, there is clearly
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When 30.0 moles of zinc reacts with excess $H_3PO_4$, how many grams of hydrogen are produced?
$3"Zn" + 2"H"_3"PO"_4 -> "Zn"_3("PO"_4)_2 + 3"H"_2$ The molar ratio of zinc: hydrogen is $3:3$ so moles of zinc = moles of hydrogen. $"m"="nM"=30xx1=30$ $"g"$
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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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How many grams of 20% zinc oxide ointment would contain 10 g of zinc oxide?
Let's check, $50*gxx20%(m_"ZnO"/m_"cream")$ $=$ $10*g$ $ZnO$. Do you know what the major use of this cream is?
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Zinc oxide reacts with hydrochloric acid to produce zinc chloride and dihydrogen monoxide. If 3.6 moles of zinc oxide reacts with an excess of hydrochloric acid, then how many grams of zinc chloride were produced?
The reaction happening in solution is the following: $ZnO(aq)+2HCl(aq)->ZnCl_2(aq)+H_2O(l)$ Since the hydrochloric acid ($HCl$) is in excess, therefore, the number of moles of Zinc oxide ($ZnO$) will determine the mass...
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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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Iron (III) oxide reacts with carbon monoxide to form molten iron and carbon dioxide. If .18 g of iron (III) oxide reacts with 0.11 g of carbon monoxide, how many grams of iron would be produced?
$"Moles of ferric oxide "=(0.18*g)/(159.69*g*mol^-1)$ $=$ $1.13xx10^-3*mol" metal oxide"$. $"Moles of carbon monoxide "=(0.11*g)/(28.0*g*mol^-1)$ $=$ $3.93xx10^-3*mol" CO"$. $Fe_2O_3$ is the reagent in deficiency (why?), and thus $2xx1.13xx10^-3*molxx55.85*g*mol^-1~=0.150*g$ iron metal are...
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If $"38 g"$ of lithium carbonate reacts with excess zinc sulfate, what mass of zinc carbonate can be produced?
$"ZnSO"_4 + "Li"_2"CO"_3"$$rarr$$"ZnCO"_3 + "Li"_2"SO"_4$ The process used to answer this question will be: $color(red)("given mass Li"_2"CO"_3"$$rarr$$color(blue)("mol Li"_2"CO"_3"$$rarr$$color(green)("mol ZnCO"_3"$$rarr$$color(purple)("mass ZnCO"_3"$ The molar masses of lithium carbonate and zinc sulfate is...
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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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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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