Question
Define atomic weight, molecular weight and equivalent weight and explain them.

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Lifetimes of the molecules in the excited states are often measured by using pulsed radiation source of duration nearly in the nano second range. If the radiation source has the duration of 2 ns and the number of photons emitted during the pulse source is 2.5 × 1015, calculate the energy of the source.
Give reasons for the following:
  1. Covalent bonds are directional bonds while ionic bonds are non- directional.
  2. Water molecule has bent structure whereas carbon dioxide molecule is linear.
  3. Ethyne molecule is linear.
The equilibrium constant for the following reaction is 1.6 ×105 at 1024K $\text{H}_2\text{ (g) + Br (g)}\rightleftharpoons2\text{HBr (g)}$ Find the equilibrium pressure of all gases if 10.0 bar of HBr is introduced into a
sealed container at 1024K.
  1. Define solubility product. Write solubility product expression for Zr3(PO4)4.
  2. Calculate the pH of 0.01 M CH3COOH solution. [Ka(CH2COOH) = 1.74 × 10-51
  3. Explain why NaCl is precipitated when HCl(g) is passed through the saturated solution of NaCl.
At 700K, equilibrium constant for the reaction:
$\text{H}_2\text{ (g) + I}_2\text{ (g)}\rightleftharpoons2\text{HI (g)}$ is 54.8. If 0.5 mol L–1 of HI(g) is present at equilibrium at 700K, what are the concentration of H2(g) and I2(g) assuming that we initially started with HI(g) and allowed it to reach equilibrium at 700K?
  1. An athlete is given 100g of glucose of energy equivalent to 1560kJ. He utilises 50% of this gained energy in the event. In order to avoid storage of energy in the body, calculate the weight of water that would need to perspire. The enthalpy of vaporisation of water is 44kJ mol-1.
  2. Compound with carbon-carbon double bond, such as ethylene, C2H4, add hydrogen in a reaction called hydrogenation, C2H4(g) + H2(g) → C2H6(g)

Calculate enthalpy change for the reaction, using the following combustion data,

$\text{C}_2\text{H}_4(\text{g})+3\text{O}_2(\text{g})\overrightarrow{\ \ \ \ \ }\ 2\text{CO}_2(\text{g})+2\text{H}_2\text{O(l)};$ $\Delta_\text{c}\text{H}^\circ=-1401\text{kJ mol}^{-1}\dots(\text{i})$

$\text{C}_2\text{H}_6(\text{g})+\frac{7}{2}\text{O}_2(\text{g})\overrightarrow{ \ \ \ \ \ \ \ }\ 2\text{CO}_2(\text{g})+3\text{H}_2\text{O(l)}$ $\Delta_\text{c}\text{H}^\circ=-1550\text{kJ mol}^{-1}\dots(\text{ii})$

$\text{H}_2(\text{g})+\frac{1}{2}\text{O}_2(\text{g})\overrightarrow{ \ \ \ \ }\ \text{H}_2\text{O(l)};$ $\Delta_\text{c}\text{H}^\circ=-286.0\text{kJ mol}^{-1}\dots(\text{iii})$

Ethyl acetate is formed by the reaction between ethanol and acetic acid and the equilibrium is represented as:
$\text{CH}_3\text{COOH (1) + C}_2\text{H}_5\text{OH (1)}\rightleftharpoons\text{CH}_3\text{COOC}_2\text{H}_5 \text{ (1) + H}_2\text{O (1)}$
At 293K, if one starts with 1.00mol of acetic acid and 0.18mol of ethanol, there is 0.171mol of ethyl acetate in the final equilibrium mixture. Calculate the equilibrium constant.
Determine the empirical formula of an oxide of iron, which has 69.9% iron and 30.1% dioxygen by mass.
$\text{K}_{\text{c}}\text{ for }\text{PCl}_5(\text{g})\rightleftharpoons\text{PCl}_3(\text{g})+\text{Cl}_2(\text{g})\text{ is }0.04\text{ at }25^\circ\text{C}.$
How much moles of PCl5 must be added to 3L flask to obtain a chlorine concentration of 0.15M.
The work function for caesium atom is 1.9 eV . Calculate (a) the threshold wavelength and (b) the threshold frequency of the radiation. If the caesium element is irradiated with a wavelength 500 nm , calculate the kinetic energy and the velocity of the rejected photoelectron.