If 4 g of NaOH dissolves in 36 g of H2O, the molarity of the solution is: (specific gravity of solution is 1 g mL-1) :
1. | 3 M | 2. | 3.5 M |
3. | 2.5 M | 4. | 2 M |
The mass of ammonia produced when 2.00 × 103 g dinitrogen reacts with 1.00 ×103 g of dihydrogen is:
1. | 2338.11 g
|
2. | 2428.57 g
|
3. | 2712.24 g
|
4. | 2180.56 g |
On complete decomposition, the volume of CO2 released at STP on heating 9.85 g of BaCO3 (atomic mass, Ba = 137) will be:
1. 1.12 L
2. 4.84 L
3. 2.12 L
4. 2.06 L
The amount of Zinc (atomic weight = 65) necessary to produce 224 mL of H2 (at STP) by the reaction with dilute sulphuric acid will be:
1. | 0.65 g | 2. | 7.6 g |
3. | 6.5 g | 4. | 8.5 g |
ln the final answer of the expression \(\large{\frac{(29.2-20.2)\times(1.79\times10^5)}{1.37}}\)
the number of significant figures after solving the expression is:
1. | 2 | 2. | 4 |
3. | 6 | 4. | 7 |
lf NA is Avogadro's number, then the number of valence electrons in 4.2 g of nitride ions (N) will be:
1. | 3.2 NA | 2. | 1.6 NA |
3. | 2.4 NA | 4. | 1.2 NA |
The weight of 1x1023 molecules of CuSO4.5H2O is:
1. 34.42 g
2. 41.42 g
3. 54.44 g
4. 68.94 g
At STP, the density of CCl4 vapour in g/L will be closest to:
1. 8.67
2. 6.87
3. 3.67
4. 4.26
The number of valence electrons present in 0.53 grams of Na2CO3 is:
1.
2.
3.
4.
1cc N2O at STP contains:
1. | \({1.32 \over 224} \times10^{23}~\text{electrons}\) | 2. | \({6.02 \over 22400} \times10^{23}~\text{molecules}\) |
3. | \({1.8 \over 224} \times10^{22}~\text{atoms}\) | 4. | All of the above |