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What bond angles are observed in $NH_4^+$, $OH_2$, $OF_2$, and $H_3O^+$?
In $NH_4^+$, the $/_H-N-H$ bond angles are $109.5$ $""^@$, as we would expect for a regular tetrahedron. $F_2O$, and $H_3O^+$ share this electronic configuration, but here the central $O$ atom...
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Oxygen reacts with fluorine to form only $OF_2$, but sulphur which is in the same group 16 as oxygen, reacts with fluorine to form $SF_2$, $SF_4$ and $SF_6$. Explain?
Indeed, oxygen can only bond with fluorine to form oxygen difluoride, $"OF"_2$. On the other hand, sulfur can easily form sulfur difluoride, $"SF"_2$, sulfur tetrafluoride, $"SF"_4$, and sulfur hexafluoride,...
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A sample of dolomitic limestone containing only $CaCO_3$ and $MgCO_3$ was analyzed. When a 0.2800 gram sample of this limestone was decomposed by heating, 75.0 mL of $CO_2$ at 750 mmHG and 20°C were evolved. How many grams of $CO_2$ were produced?
We use the Ideal Gas equation to access the moles of carbon dioxide evolved: $n=(PV)/(RT)$ $=$ $((750*mm*Hg)/(760*mm*Hg*atm^-1)xx75.0xx10^-3*L)/(0.0821*L*atm*K^-1*mol^-1xx293*K)$ $=3.1xx10^-3mol$. $"Mass of carbon dioxide produced"=3.1xx10^-3molxx44.0*g*mol^-1=??g$ The key to doing this problem was...
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What is the oxidation number of oxygen in $OF_2(g)$?
Oxidation state is the charge left on the central atom, when all the pairs of electrons are removed from the central atom, with the charge assigned to the most electronegative...
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How many molecules are present in a $27*g$ mass of $OF_2(g)$?
Where $N_A="Avogadro's number"$ $=$ $6.022xx10^23*mol^-1$ $"Number of moles"$ $=$ $"Mass"/"Molar mass"$ $=$ $(27*g)/(54.00*g*mol^-1)=0.500*mol$ And thus $"Number of molecules"$ $=$ $6.022xx10^23*mol^-1$ $=$ $3.011xx10^23$ $OF_2$ molecules.......... What is the oxdation number of...
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If 3.00 mol of $CaCO_3$ undergo decomposition from $CaO$ and $CO_2$ how many grams of $CO_2$ are produced?
We need the stoichiometric equation; $CaCO_3(s) + Delta rarr CaO(s) + CO_2(g)uarr$ You have to heat this fairly fiercely, but clearly, quantitative reaction indicates that 1 mol of carbon dioxide...
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For $CH_4 +2O_2 -> CO_2 + 2H_2O$, the molar mass of oxygen gas ($0_2$) is 32.00 g/mol. The molar mass of carbon dioxide ($CO_2$) is 44.01 g/mol. What mass of $CO_2$, in grams, will form when 8.94 g $O_2$ completely react?
The balanced chemical equation tells us unequivocally that 16 g of methane gas reacts with 32 g of dioxygen gas to give 44 g of carbon dioxide, and 36 g...
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What is the limiting reagent and the moles of $CO_2$ formed when 11 moles $CS_2$ reacts with 18 moles $O_2$ to produce $CO_2$ gas and $SO_2$ gas at STP?
Limiting reagent problems are all about using the that exists between the reactants to determine if you have enough of each reactant to allow for their complete consumption....
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$CO_2$ gas, in the dry state, may be produced by heating calcium carbonate. $CaCO_3 (s)DeltaCaO(s) + CO_2(g)$. What volume of $CO_2$, collected dry at 55 C and a pressure of 774 torr, is produced by complete thermal decomposition of 10.0 g of $CaCO_3$?
$10gramsCaCO_3(s) => CaO(s) + (?)O_2(g)$ $"moles" CaCO_3 = ((10g)/(100(g/(mol))))$ = $0.10"mole"$ From reaction ratios => moles $CaCO_3(s)$ consumed = moles $O_2(g)$ produced = 0.10 mole $(O_2(g))$**** If a 'dry'...
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The concentration of $CO_2$ in a can of soda is approximately 0.045 M. If all of the $CO_2$ in a 12 ounce soda evolves from solution, how many liters would the $CO_2$ gas take up at STP?
The idea here is that you need to figure out how many moles of carbon dioxide, $"CO"_2$, are initially dissolved in the soda by using the volume and of...
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