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hram777 [196]
3 years ago
11

Which increases the rate of a chemical reaction? A. a catalyst B. a higher volume C. a lower pressure D. a lower temperature

Chemistry
2 answers:
Tanya [424]3 years ago
6 0
A. A catalyst because it increases the time that it takes to happen
taurus [48]3 years ago
3 0
A catalyst will increase the rate of a chemical reaction by changing the reaction mechanism so that the reaction has a lower activation energy.  

a higher volume will decrease the concentrations which will intern decrease the number of collisions which will slow down the rate of the reaction since collisions between reactants are what make reactions happen.  A lower temperature causes the molecules to slow down thereby lowering the collision rate which will lower the reaction rate.  A lower pressure will lower the number of collisions which will intern result in a lower reaction rate (this can be thought of as a lower concentration since lower pressures involve less gas per unit volume)
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How does aspirin interact with other drugs
Damm [24]

The most common drugs that aspirin may interact with are: Anti-inflammatory painkillers, such as diclofenac, ibuprofen, indomethacin, and naproxen. Taken with aspirin, these can increase the risk of bleeding. Warfarin, an anticoagulant drug, or a blood thinner, which stops the blood from clotting.

7 0
3 years ago
Given a fixed amount of gas held at constant pressure, calculate the volume it would occupy if a 2.00 L sample were cooled from
aliina [53]

Answer:

1.82 L

Explanation:

We are given the following information;

  • Initial volume as 2.0 L
  • Initial temperature as 60.0°C
  • New volume as 30.0 °C

We are required to determine the new volume;

From Charles's law;

\frac{V_1}{T_1}=\frac{V_2}{T_2}

Where, V_1 and V_2 are initial and new volume respectively, while T_1 and T_2 are initial and new temperatures respectively;

T_1= 333 K

T_2=303K

V_1 =2.0L

Rearranging the formula;

V_2=\frac{V_1T_2}{T_1}

    = \frac{(2.0L)(303K)}{333K} \\=1.820 L

Therefore, the new volume that would be occupied by the gas is 1.82 L

7 0
3 years ago
Ibuprofen is a common pain reliever and anti-inflammatory. Its formula is C13H18O2. What percent by mass of ibuprofen is the car
Anarel [89]

Answer:

Explanation:

%Carbon =  mass of carbon / mas of C13H18O2) X100%

             =      13X12/ (13X12+18+2X16)X100%

           =    156/206) X100%= 75.7%

8 0
2 years ago
In the Haber process for ammonia synthesis, K " 0.036 for N 2 (g) ! 3 H 2 (g) ∆ 2 NH 3 (g) at 500. K. If a 2.0-L reactor is char
lisabon 2012 [21]

Answer : The partial pressure of N_2,H_2\text{ and }NH_3 at equilibrium are, 1.133, 2.009, 0.574 bar respectively. The total pressure at equilibrium is, 3.716 bar

Solution :  Given,

Initial pressure of N_2 = 1.42 bar

Initial pressure of H_2 = 2.87 bar

K_p = 0.036

The given equilibrium reaction is,

                              N_2(g)+H_2(g)\rightleftharpoons 2NH_3(g)

Initially                   1.42      2.87             0

At equilibrium    (1.42-x)  (2.87-3x)     2x

The expression of K_p will be,

K_p=\frac{(p_{NH_3})^2}{(p_{N_2})(p_{H_2})^3}

Now put all the values of partial pressure, we get

0.036=\frac{(2x)^2}{(1.42-x)\times (2.87-3x)^3}

By solving the term x, we get

x=0.287\text{ and }3.889

From the values of 'x' we conclude that, x = 3.889 can not more than initial partial pressures. So, the value of 'x' which is equal to 3.889 is not consider.

Thus, the partial pressure of NH_3 at equilibrium = 2x = 2 × 0.287 = 0.574 bar

The partial pressure of N_2 at equilibrium = (1.42-x) = (1.42-0.287) = 1.133 bar

The partial pressure of H_2 at equilibrium = (2.87-3x) = [2.87-3(0.287)] = 2.009 bar

The total pressure at equilibrium = Partial pressure of N_2 + Partial pressure of H_2 + Partial pressure of NH_3

The total pressure at equilibrium = 1.133 + 2.009 + 0.574 = 3.716 bar

6 0
3 years ago
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blondinia [14]

Answer:

the answer would be (A.) and (D.).

Explanation:

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3 years ago
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