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When 3.0 g of carbon is burnt in 8.0 g of oxygen, 11.0 g of carbon dioxide is produced. what is the mass of carbon dioxide will be formed when 3.0 g of carbon is burnt in 50.0 g of oxygen? Which law of chemical combination will govern the answer?
When a $3.0*g$ mass of carbon is burnt in an $8.0*g$ mass of dioxygen, the carbon and the oxygen are stoichiometrically equivalent. Of course, the combustion reaction proceeds according to...
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Which equation is correctly balanced:
$A.$ $Al(s) + 3O_2(g) rarr Al_2O_3(s);$
$B.$ $Al(s) + 3O_2(g) rarr Al_2O_3(s);$
$C.$ $Al(s) + 3/2O_2(g) rarr Al_2O_3(s);$
$D.$ $2Al(s) + 3O_2(g) rarr 2Al_2O_3(s)?$
Alumina is $Al_2O_3$, which is the product of aluminum oxidation. None of your equations shows the correct formulae. We can rewrite the correct equation as: $2Al(s)+ 3/2O_2(g) rarr Al_2O_3(s)$ This...
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When burning 180 g glucose in the presence of the 192 g of oxygen, water and carbon dioxide are produced. If 108 g of water is produced, how much carbon dioxide is produced?
We're asked to find the mass of $"CO"_2$ produced in a given reaction, given that $108$ $"g H"_2"O"$ is formed. What we can do first is write the balanced chemical...
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You are given 4.5 moles of $O_2$ to react with $1.60 x10^2$ g $C_2H_4$. Upon completion of the reaction, will there be any remaining $C_2H_4$?
We represent the combustion of ethylene by this reaction: $H_2C=CH_2(g) +3O_2(g) rarr 2CO_2(g) + 2H_2O(l)$ For complete combustion, $28*g$ of ethylene thus requires $96*g$ of dioxygen. Here, $"moles of ethylene"$...
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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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In the reaction $2NaOH+H_2SO_4 -> 2H_2O+Na_2SO_4$, how many grams of sodium sulfate will be formed if you start with 200.0 grams of sodium hydroxide and you have an excess of sulfuric acid?
Given the molecular weights: $Mr_(NaOH)=40 g/(mol)$ $Mr_(Na_2SO_4)=142 g/(mol)$ The analogy of the moles will be held constant: $n_(NaOH)/n_(Na_2SO_4)=2/1$ $n_(NaOH)/n_(Na_2SO_4)=2$ For each one, substitute: $n=m/(Mr)$ Therefore: $n_(NaOH)/n_(Na_2SO_4)=2$ $(m_(NaOH)/(Mr_(NaOH)))/(m_(Na_2SO_4)/(Mr_(Na_2SO_4)))=2$ $(200/40)/(x/142)=2$ $(200*142)/(40x)=2$ $200*142=2*40x$...
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In the reaction $C_2H_4(g)+3O_2(g)->2CO_2(g)+2H_2O(g)$, if 2.70 mol $C_2H_4$ is reacted with 6.30 mol $O_2$, what is the limiting reagent?
Why can I say "clearly"? The stoichiometric equation you have posted shows that 1 mole of ethylene requires 3 moles of oxygen gas (the diatomic molecule). Thus, 2.70 mol ethylene...
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How many moles of ethylene ($C_2H_4$) can react with 12.9 liters of oxygen gas at 1.2 atmospheres and 297 Kelvin?
Start by using the ideal gas equation to figure out the the number of moles $O_2$ used. $ P*V= n*R*T$ Where $P" "$ is the pressure expressed in atm. $V"...
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The solubility of carbon dioxide in water is 0.161 g $CO_2$ in 100 mL of water at 20°C and 1.00 atm. A soft drink is carbonated with carbon dioxide gas at 5.50 atm pressure. What is the solubility of carbon dioxide in water at this pressure?
$"8.855 g/L"$ This is just asking you to calculate the new molar (i.e. molar solubility) at a different pressure, i.e. use the . (We'll end up converting...
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Given $2CO(g) + O_2(g) rarr 2CO_2(g)$ $DeltaH^@=-564*kJ*mol^-1$...what is the enthalpy associated with the formation of a mass of $44.0*g$ of carbon dioxide by these means?
$"2CO +O"_2rarr"2CO"_2$ $;DeltaH^@=-564*kJ*mol^-1$ $DeltaH^@$ is always quoted per mole of reaction as written. That is synthesis of 2 moles of carbon dioxide from 2 moles of carbon monoxide and...
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