Heat required= mass of copper × specific heat of copper × change in temperature1000J = mass of copper× 0.40 J/g C × 25CMass of copper = 100g
1 Answers 1 views4.08=2.28?= 1= 4.08/2.28= 1.79g
1 Answers 1 viewsBegin by determining the molar mass of each compound involved in the reaction. Using atomic masses from the periodic table, we will find the quantity of moles of each element...
1 Answers 1 viewsMg + CuSO4 = MgSO4 + Cu n(Mg) = m/M M(Mg) = 24 g/mol n(Mg) = 10g/24g/mol = 0.417 mol n(CuSO4) = m/M M(CuSO4)= 64 + 32 + 16*4 =...
1 Answers 1 viewsAt the temperature of sulphur dioxide decomposition, i.e. over 4300 K.
1 Answers 1 viewsBalanced reaction equation:2Al + 3CuSO4 = 3Cu + Al2(SO4)3Molar weight of Al: 26.98 g/molQuantity of Al: 10.45 g / 26.98 g/mol = 0.387 molMolar weight of CuSO4: 159.61 g/molQuantity of...
1 Answers 1 viewsamount of heat = q = 4000 J;T1 = 98℃;T2 = 199℃;change in temperature = ΔT = T2 - T1 = 199℃ - 98℃ = 101℃;specific heat of Cu =...
1 Answers 1 viewsA molar mass of X3PO4 equals:Mr(X3PO4) = (3 × 46.31 g/mol) + 31 g/mol + (3 × 16 g/mol) = 217.93 g/molThe percentage composition by mass of X in X3PO4...
1 Answers 1 views2Cu2O + Cu2S -> 6Cu + SO2n= m/Mn(Cu2O)= 250000g/143.09g/mol= 1747 moln(Cu2S)= 129000g/ 159.16 g/mol= 810.5 molFind limiting reactant: compare1747/2 and 810.5873.5>810.5, consequently , Cu2S is a limiting reactant.According to equation...
1 Answers 1 viewsWhile combustion of 1 mol of sulfur 297kJ/mol is released.From a given mass we found actual number of moles: n=m/M.n=6.4/32=0.2 (moles).∆H=0.2×(-297)=-59.4 (kJ/mol).
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