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Nostrana [21]
3 years ago
10

In nature, oxygen has three common isotopes. The atomic masses and relative abundances of these isotopes are given in the table

below.
Isotope Atomic Mass (amu) Relative Abundance
O-16          15.995                          99.759%
O-17          16.995                             0.037%
O-18          17.999                               0.204%
Calculate the average atomic mass of oxygen. Show all of your calculations below.
Chemistry
1 answer:
Reil [10]3 years ago
7 0
<span>15.995* 0.99759 + 16.995*0.00037 + 17.999*0.00204 = 15.999</span>
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Water flows from the bottom of a large tank where the pressure is 100 psig through a pipe to a turbine which produces 5.82 hp. T
Marianna [84]

Explanation:

Bernoulli equation for the flow between bottom of the tank and pipe exit point is as follows.

   \frac{p_{1}}{\gamma} + \frac{V^{2}_{1}}{2g} + z_{1} = \frac{p_{2}}{\gamma} + \frac{V^{2}_{2}}{2g} + z_{2} + h_{f} + h_{t}

    \frac{(100 \times 144)}{62.43} + 0 + h[tex] = [tex]\frac{(50 \times 144)}{(62.43)} + \frac{(70)^{2}}{2(32.2)} + 0 + 40 + 60

                          h = \frac{(50 \times 144)}{(62.43)} + \frac{(70)^{2}}{2(32.2)} + 40 + 60 - \frac{(100 \times 144)}{(62.43)}

                            = 60.76 ft

Hence, formula to calculate theoretical power produced by the turbine is as follows.

                                 P = mgh

                                     = 100 \times 60.76

                                     = 6076 lb.ft/s

                                     = 11.047 hp

Efficiency of the turbine will be as follows.

                \eta_{t} = \frac{P_{actual}}{P_{theoretical}} × 100%

                                = \frac{5.82}{11.047} \times 100%                      

                                = 52.684%

Thus, we can conclude that the efficiency of the turbine is 52.684%.

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3 years ago
Question # 10
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Determine the rate law, including the values of the orders and rate law constant, for the following reaction using the experimen
olga55 [171]

Answer: Rate law=k[A]^1[B]^2, order with respect to A is 1, order with respect to B is 2 and total order is 3. Rate law constant is 3L^2mol^{-2}s^{-1}

Explanation: Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

Rate=k[A]^x[B]^y

k= rate constant

x = order with respect to A

y = order with respect to A

n = x+y = Total order

a) From trial 1: 1.2\times 10^{-2}=k[0.10]^x[0.20]^y    (1)

From trial 2: 4.8\times 10^{-2}=k[0.10]^x[0.40]^y    (2)

Dividing 2 by 1 :\frac{4.8\times 10^{-2}}{1.2\times 10^{-2}}=\frac{k[0.10]^x[0.40]^y}{k[0.10]^x[0.20]^y}

4=2^y,2^2=2^y therefore y=2.

b) From trial 2: 4.8\times 10^{-2}=k[0.10]^x[0.40]^y    (3)

From trial 3: 9.6\times 10^{-2}=k[0.20]^x[0.40]^y   (4)

Dividing 4 by 3:\frac{9.6\times 10^{-2}}{4.8\times 10^{-2}}=\frac{k[0.20]^x[0.40]^y}{k[0.10]^x[0.40]^y}

2=2^x,2=2^1, x=1

Thus rate law is Rate=k[A]^1[B]^2

Thus order with respect to A is 1 , order with respect to B is 2 and total order is 1+2=3.

c) For calculating k:

Using trial 1:  1.2\times 10^{-2}=k[0.10]^1[0.20]^2

k=3 L^2mol^{-2}s^{-1}.



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