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A gas exerts a pressure of 2.0 atm, at 30°C, in a 10 L container. In what size container would the same amount of gas exert a pressure of 4.0 atm at 20° C?
Using the gas law: pV = nRT, and keeping the same number of moles of gas (n),we find the final volume V2:V2 = (T2/p2)*(p1*V1/T1) = (293 K/ 4.0 atm)*(2.0 atm...
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When 25.0 mL of 0.25 mol/L LiOH and 25.0 mL of 0.25 mol/L HCl are mixed together, the temperature warms 15.8o C. What is the molar enthalpy of neutralization for LiOH? (3 marks)
528528.96 J/mol
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the heat of neutralisation of lioh and hcl at 25*c is 34.868 kj/mol heat of ionisation of lioh will be
Solution. Regardless of the nature of the strong base and strong acid, the heat of neutralization of dilute solutions goes with the release of 55.9 kJ / mol of heat....
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If the total air pressure is 1.05 atm, the partial pressure of carbon dioxide is 0.08 atm, and the partial pressure of hydrogen sulfide is 0.05 atm, what is the partial pressure of the remaining air?
As we know, Total pressure is the sum of partial pressure of individual gases.PT = 1.05 -(0.08+0.05+Pair)Pair = [0.92] atm
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your teacher makes a solution from LiOH. 5.03 grams of LiOH is mixed into 1.27 of water. From this information calculate the concentration of the solution
The mass concentration of the substance: the mass of the substance divided by the volume of the mixture: Cm = m/V (volume of LiOH is omitted in the total volume...
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The temperature of a gas is 298.0 k when the pressure is 4.00 atm. At the same volume, what is the temperature at which the pressure of the gas is 3.0 atm
1 = 298 K P1 = 4 atm P2 = 3 atm Gay-Lussac`s Law: P1/T1 = P2/T2 T2 = T1*P2/P1 = 298K*3atm/4atm = 223.5 K
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4 mol of gas is measured at 4 atm pressure to have a volume of 3 L, a temperature of 270 K. If the conditions change such that there are 3 mol at 2 atm and at 300 K, what is the new volume?
Pressure, temperature and number of moles of the gas have changed so According to ideal gas equation PV = nRTFrom that we can write P1V1 / n1T1 = P1V1 /...
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At standard temperature and pressure (0 ∘C and 1.00 atm ), 1.00 mol of an ideal gas occupies a volume of 22.4 L. What volume would the same amount of gas occupy at the same pressure and 95 ∘C ?
P1 = P2 = 1.00 atm = constant;V1 = 22.4 L;T1 = 0 °C = 273.15 K;T2 = 95 °C = 368.15 K;V2 = unknown;Solution:(P1×V1)/(T1) = (P2×V2)/(T2);P1 = P2 =...
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Consider a container with 9.05g of N2 gas and an unknown mass of CO2 gas. If we know that the partial pressure of the CO2 is twice that of the N2, determine the mass of CO2 gas in the container.
P is proportional to nPco2/PN2 = nco2/nN2Moles of gas is equal to the weight/molecular weight of gasPco2 is twice that of PN2Pco2 = 2PN2, weight of N2 = 9.05 gram2PN2/PN2...
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Consider a container with 5.08g of N2 gas and an unknown mass of CO2 gas. If we know that the partial pressure of the CO2 is twice that of the N2, determine the mass of CO2 gas in the container
Mass of nitrogen= 5.08 gNo.of mole of nitrogen= 5.08/28= .182Partial pressed of nitrogen let = PPV=nRTV=.182RT/PIn case of carbon dioxideMass of carbon dioxide=?Partial pressure of carbon dioxide= 2PPV=nRTn=PV/RTn=2P×.182RT/PRTn=.364 Mass of...
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