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Q. No.For a reaction, \(A + B \rightarrow \text {Product}\), the rate is given by,
\(r = k[A]^{{1/2}}[B]^2\)
What is the order of the reaction?
1. 0.5
2. 2
3. 2.5
4. 1
\(r = k[A]^{{1/2}}[B]^2\)
What is the order of the reaction?
1. 0.5
2. 2
3. 2.5
4. 1
Subtopic: Β Definition, Rate Constant, Rate Law |
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The rate of a reaction is expressed in different ways as follows
The reaction is:
1. 4π΄ + π΅ → 2πΆ + 3π·
2. π΅ + 5π· → 3π΄ + 2πΆ
3. 4A +2B →2C +3D
4. B + \(\frac 12\)D → 4A →2C
Subtopic: Β Definition, Rate Constant, Rate Law |
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One of the steps in the manufacture of nitric acid is the oxidation of ammonia shown in this equation.
4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g)
If gaseous water appears at a rate of 0.025 mol·min–1, at what rate does ammonia disappear?
1. 0.0040 mol·min–1
2. 0.017 mol·min–1
3. 0.038 mol·min–1
4. 0.150 mol·min–1
4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g)
If gaseous water appears at a rate of 0.025 mol·min–1, at what rate does ammonia disappear?
1. 0.0040 mol·min–1
2. 0.017 mol·min–1
3. 0.038 mol·min–1
4. 0.150 mol·min–1
Subtopic: Β Definition, Rate Constant, Rate Law |
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For the reaction N2 + 3H2 2NH3, the rate = 2x10-4 Ms-1 .Therefore, the rate is given as:
(1) 10-4 Ms-1
(2) 104 Ms-1
(3) 10-2 sM-1
(4) 10-4 sM-1
Subtopic: Β Definition, Rate Constant, Rate Law |
Β 91%
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The rate of a chemical reaction doubles for every 10°C increase in temperature.
If the temperature is raised by 50°C, by what factor does the rate of the reaction increase?
1. 10 times
2. 24 times
3. 32 times
4. 64 times
Subtopic: Β Definition, Rate Constant, Rate Law |
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The rate law for the reaction :
RCl + NaOH (aq) → ROH + NaCl
is given by, Rate = k1[RCl].
The rate of the reaction will be:
RCl + NaOH (aq) → ROH + NaCl
is given by, Rate = k1[RCl].
The rate of the reaction will be:
| 1. | Doubled on doubling the concentration of sodium hydroxide. |
| 2. | Halved on reducing the concentration of alkyl halide to one half. |
| 3. | Decreased on increasing the temperature of the reaction. |
| 4. | Unaffected by increasing the temperature of the reaction. |
Subtopic: Β Definition, Rate Constant, Rate Law |
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Which of the following expression is correct for the reaction given below?
\(2 \mathrm{HI}_{(g)} \rightarrow \mathrm{H}_{2(g)}+\mathrm{I}_{2(g)}\)
\(2 \mathrm{HI}_{(g)} \rightarrow \mathrm{H}_{2(g)}+\mathrm{I}_{2(g)}\)
| 1. | \(\dfrac{-\Delta[\mathrm{H}I]}{\Delta t}=\dfrac{2 \Delta\left[\mathrm{H}_2\right]}{\Delta t}\) | 2. | \(\dfrac{-\Delta[\mathrm{HI}]}{\Delta t}=\dfrac{4\Delta\left[\mathrm{I}_2\right]}{\Delta t}\) |
| 3. | \(\dfrac{-\Delta[\mathrm{HI}]}{\Delta t}=\dfrac{4 \Delta\left[\mathrm{H}_2\right]}{\Delta t}\) | 4. | \( \dfrac{-\Delta[\mathrm{HI}]}{\Delta t}=\dfrac{\Delta\left[\mathrm{H}_2\right]}{\Delta t}\) |
Subtopic: Β Definition, Rate Constant, Rate Law |
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NEET - 2024
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Consider a zero-order reaction. The rate equation for the given expression \(2X + Y \rightarrow Z\) is:
1. Rate = \(k[X][Y]\)
2. Rate = \(k[X]^0[Y]^0\)
3. Rate = \(k[X]^0[Y]\)
4. Rate = \(k[X][Y]^0\)
1. Rate = \(k[X][Y]\)
2. Rate = \(k[X]^0[Y]^0\)
3. Rate = \(k[X]^0[Y]\)
4. Rate = \(k[X][Y]^0\)
Subtopic: Β Definition, Rate Constant, Rate Law |
Β 90%
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Given a general reaction, \(A + 2B \rightarrow C + D\)
The correct statement among the following is:
The correct statement among the following is:
| 1. | Rate of disappearance of A = Rate of disappearance of B. |
| 2. | Rate of disappearance of A = 1/2 Rate of appearance of C. |
| 3. | Rate of disappearance of A = 1/2 Rate of disappearance of B. |
| 4. | Rate of disappearance of A = 1/2 Rate of appearance of D. |
Subtopic: Β Definition, Rate Constant, Rate Law |
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For the chemical reaction of the type
\(2A\rightarrow\frac12B~\)
the correct relationship amongst the rate expressions is:
1. \(-2\frac{d[A]}{dt}=+\frac12\frac{d[B]}{dt} \)
2. \(+2\frac{d[A]}{dt}=-\frac12\frac{d[B]}{dt} \)
3. \(-\frac12\frac{d[A]}{dt}=+2\frac{d[B]}{dt} \)
4. \(+\frac12\frac{d[A]}{dt}=-2\frac{d[B]}{dt} \)
\(2A\rightarrow\frac12B~\)
the correct relationship amongst the rate expressions is:
1. \(-2\frac{d[A]}{dt}=+\frac12\frac{d[B]}{dt} \)
2. \(+2\frac{d[A]}{dt}=-\frac12\frac{d[B]}{dt} \)
3. \(-\frac12\frac{d[A]}{dt}=+2\frac{d[B]}{dt} \)
4. \(+\frac12\frac{d[A]}{dt}=-2\frac{d[B]}{dt} \)
Subtopic: Β Definition, Rate Constant, Rate Law |
Β 90%
Level 1: 80%+
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