carbon react with chlorine to form ccl4 .36gm of carbon was mixed with 142gmof ccl2.calculate mass of ccl4 produce and remaining mass of reactant
Asked by aliadil96935 | 16th Feb, 2020, 05:46: PM
The reaction is;
C + 2Cl2 → CCl4
12 g 4×35.5g
The mass of chlorine is less than required to formed CCl4
Therfeore, chlorine is the limiting reagent.
142 g of Cl2 reacts with 12 g of Carbon.
So, mass of carbon is in excess.
142 g of Cl2 gives 154 g of CCl4
Therefore mass of CCl4 produced is 154 gm.
Mass of carbon left = 36 − 12 = 24 gm
Mass of chlorine left = 0 gm
Answered by Varsha | 17th Feb, 2020, 10:40: AM
- 25ml of a solution containing HCl was treated with excess of M/5 KIO3 and KI solution of unknown concentration where I2 liberated is titrated against a standard solution of 0.021M Na2S2O3 solution whose 24ml were used up. Find the strength of HCl and volume of KIO3 solution consumed.
- Phosphorus pentachloride decomposes according to this equation. PCl5(g) equilibrium reaction arrow PCl3(g) + Cl2(g) An equilibrium mixture in a 5.00 L flask at 245°C contains 4.27 g of PCl5, 9.31 g of PCl3, and 2.86 g of Cl2. How many grams of each will be found if the mixture is transferred into a 2.00 L flask at the same temperature.
- What is Gram Atomic Mass?
- Calculate the mass of potassium chlorate required to liberate 6.72dmcube of oxygen at step.Molar mass of potassium chlorate is 122.5g mol inverse Ans.24.5g
- Air contains 20% oxygen by volume how much volume of air will be required for combustion of 100 cc acetylene Why we use at last as 100/20*250
- When 200 cm cube of ethylene is burnt in sufficient air to form CO2 and steam and all measurements are made at constant pressure and 100 °C how do we calculate unreacted air?
- A compoundmade up of two elements A and B has A=70%,B=30 Their relative number of moles in compound is 1.25 and 1.88, calculate: [ i ] Atomic masses of the elements A and B [ ii ] Molecular formula of the compond,if its molecular mass is found to be 160.
- 1 mole of ferric oxalate is oxidized by x mole of MnO4- and also 1 mole of ferrous oxalate is oxidized by y mole of MnO4- in acidic medium . The ratio (x/y) is : (a) 2:1 (b) 1:2 (c) 3:1 (d) 1:3
- The decomposition of a certain mass of CaCO3 gave 11.2 dm3 of CO2 gas at STP . The mass of KOH required to completely neutralise the gas is a) 56g b) 28g c) 42g d)20g
Kindly Sign up for a personalised experience
- Ask Study Doubts
- Sample Papers
- Past Year Papers
- Textbook Solutions
Verify mobile number
Enter the OTP sent to your number