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What phase changes, if any, occur if carbon dioxide initially at -80 degrees celsius and 8.0 atm is allowed to warm to -25 degrees celsius at 5.0 atm?
Using law PV = nRT, you can see, that if n,R = const, and T and P are used for some processes,V-volume is the one,that can be changed.
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10g of calcium carbonate reacted with phosphoric acid to produce calcium phosphate, water and carbon di oxide. write a balanced chemical equation
Balanced chemical equation for this reaction is: 3CaCO3(s) + 2H3PO4(l) = Ca3(PO4)2(s) + 3H2O(aq) + 3CO2(g)
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What mass of calcium oxide, CaO, forms when 28g calcium carbonate, CaCO3, decomposes on heating?
CaCO3 = CaO+CO2n (CaO)=n(CaCO3)n=m/MM(CaCO3)=100 g/molM(CaO)=56 g/moln(CaCO3)=28/100=0.28 moln (CaO)=n(CaCO3)=0.28 molm (CaO)=n x M = 0.28 x 56 = 15.7 g
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Solid calcium carbonate is heated and decomposes to solid calcium oxide and carbon dioxide gas.
Solution:Word equation:Solid calcium carbonate is heated and decomposes to solid calcium oxide and carbon dioxide gas.The balanced molecular equation:CaCO3(s) → CaO(s) + CO2(g)
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Calcium carbonate decomposes to form calcium oxide and carbon dioxide on strong heating. What is the volume of carbon dioxide released, measured at r.t.p, when 10.5 g of calcium oxide is formed?
CaCO3 = CaO + CO2 nCO2 = nCaCO3 = mCaCO3/MWCaCO3 = 10.5 g/100.0869 g/mol = 0.1049 mol; VCO2 = nCO2*Vm = 0.1049 mol*24 L/mol = 2.5178 L ≈ 2.52 L
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A sample of an ideal gas has a volume of 3.60 L at 13.40 degrees Celsius and 1.30 atm. What is the volume of gas at 24.60 degrees Celsius and 0.990 atm
Combined gas Law P1V1 / T1 = P2V2 / T2 P1 = 1.30 atm V1 = 3.60 L T1 (must be in Kelvin = 13.40 deg C + 273.15) =...
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Ten grams of calcium carbonate was produced when carbon dioxide was added to lime water (calcium hydroxide in solution). What volume of carbon dioxide at STP was needed
CO2 + Ca(OH)2 = CaCO3 + H2Om(CaCO3) = 10.0 g(10 g CaCO3 / 1)(1 mol / 100.1 g)(1 mol CO2 / 1 mol CaCO3)(22.4 L STP / 1 mol) = 2.24 L CO2 STP
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Solid calcium carbonate decomposed to produce solid calcium oxide and carbon dioxide gas. Express your answer as a chemical equation.
CaCO3 (s) = CaO (s) + CO2 (g)
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A volume of carbon dioxide gas equals 20.0 L was collected at 23 degrees celsius and 1.00 atm pressure. what would be the volume of carbon dioxide collected at 23 celsius and 0.830 atm?
General gas equation:p1*V1/T1=p2*V2/T2p1= 1atmV1= 20 LT1=T2=23 oCp2=0.83 atmV2 - ?V2=p1*V1/p2 = 20/0.83 = 24.1 LAnswer: 24.1 L
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What is the mass in grams of 11.5 l of N2 at 48.2 degree Celsius and 582mmHg?
How many moles of NO2 gas have a volume of 1,311.4 at 8.1 degree Celsius and 2.8 atm pressure?
1.PV= nRT. 582mmHg to atm = 582/760 = 0.76579atm T = 48.2+273 = 321.2Kn= PV/RT = 0.76579 × 11.5 / (0.0821 × 321.2) = 0.33molMole = mass/molar massMass = mole...
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