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And in Scotland (where there are notable dipsos!) it is
And thus is molar terms, we simply turn the mass into a molar quantity:
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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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How many kilojoules of heat are required to vaporize 50.0 g of ethanol, $C_2H_6O$? The boiling point of ethanol is 78.3°C. Its molar heat of vaporization is 38.6 kJ/mol.
$"H"_3"CCH"_2"OH"(l) +Delta rarr "H"_3"CCH"_2"OH"(g)$ You have a mass of $50.0*g$ $"EtOH"$, that is assumed to be at $78.3$ $""^@C$, and the enthalpy of vaporization is calculated by the product: $DeltaH_"vaporization"^@=(50.0*g)/(46.07*g*mol^-1)xx38.6*kJ*mol^-1=$...
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Find the partial pressure in a solution containing ethanol and 1-propanol with a total vapor pressure of $"56.3 torr"$? The pure vapor pressures are $"100.0 torr"$ and $"37.6 torr"$, respectively, and the solution has a mol fraction of $0.300$ of ethanol.
Consider Raoult's law compared with Dalton's law of partial pressures: $P_i = overbrace(chi_(i(l))P_i^"*")^"Raoult's Law" = underbrace(chi_(i(v))P_"tot")_"Dalton's Law"$, where: $P_i$ is the partial vapor pressure of component $i$, i.e....
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Which solution contains the biggest amount, in mol, of chloride ions?
A. 20 cm3 of 0.50 mol dm−3 NH4Cl
B. 60 cm3 of 0.20 mol dm−3 MgCl2
C. 70 cm3 of 0.30 mol dm−3 NaCl
D. 100 cm3 of 0.30 mol dm−3 ClCH2COOH
And to answer the question, we must calculate the of of each solution with respect to chloride ions. And $"number of moles"="concentration"xx"volume"$ For $(a):$ there are $0.020*dm^3xx0.50*mol*dm^-3=0.01*mol$. For $(b):$ $0.060*dm^3xx0.20*mol*dm^-3xx"2...
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You have 1 L of 100 proof (50% V/V) Scotch whisky (ethanol, $C_2H_5OH$). Calculate the molarity, the mole fraction, the molality of the ethanol and if the temperature drops to -10C could you still drink the whisky? Density of ethanol =0.79g/ml kf=-1.86C/m
!! LONG ANSWER !! The first thing you need to do is determine exactly how much ethanol your 1-L sample contains. Since you're dealing with a 50% v/v solution,...
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A bottle of wine contains 12.5% ethanol ($CH_3CH_2OH$) by volume. The density of ethanol is 0.789 g/cm^3 and the density water is 1.000 g/cm^3. How do you calculate the concentration of ethanol in terms of mass percent of ethanol?
Percent of alcohol by volume (ABV) is the volume of ethanol in $"100 cm"^3$ of solution. It is impossible to answer this question because we don’t know the volume or...
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Mole fraction of ethanol in ethanol and water mixture is 0.25. Hence percentage concentration of ethanol by weight of mixture is?
I'll show you two methods that you can use to solve this problem. $color(white)(a)$ THE MORE TEDIOUS APPROACH $color(white)(a)$ As you know, a solution's by mass tells you...
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At some temperature, a 100-L reaction vessel contains a mixture that is initially 1.0 mol Co and 2.0 mol H2. The vessel also contains a catalyst so that the following equilibrium is attained:
CO(g) + 2H2(g) <--> CH3OH(g)
At equilibrium, the mixture contains 0.100 mol CH3OH. In a later experiment in the same vessel, you start with 1.0 mol CH3OH. How much methanol is there at equilibrium?
Methanol's concentration at equilibrium is $0.001M$. Before solving for the concentration, try and intuitively imagine what will happen. Since the second experiment is done under the same conditions as the...
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$(i)$ What volume of $5.00*mol*L^-1$ $HCl(aq)$ is required to react with a $17.0*g$ mass of sodium hydroxide. $(ii)$ what volume of sodium sulfide at $0.100*mol*L^-1$, is required to precipitate a $33.0*mL$ volume of $0.100*mol*L^-1$ of $AgNO_3$?
Our basic equation is...... $"Concentration"="Moles of solute"/"Volume of solution"$. And thus by taking a product or a quotient, we can get the number of moles or the volume of solution....
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If the temperature of 34.4 g of ethanol increases from 25 °C to 78.8 °C, how much heat has been absorbed by the ethanol? The specific heat of ethanol is 2.44 J/(gC)?
Use the following formula: $q=mcDeltat$, where $q$ is energy in Joules, $m$ is mass, $c$ is capacity, and $Deltat$ is change in temperature: $Deltat=(T_"final"-T_"initial")$ Organize your data: Known $m="34.4 g"$...
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