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2 years ago

3S8 + 8 OH- + 8 S3 + 4 HOOH

Chemistry

1 answer:

NemiM [27]2 years ago

4 0

Answer:

Second order

Explanation:

We could obtain the order of reaction by looking at the table very closely.

Now notice that in experiment 1 and 2, the concentration of [OH^-] was held constant while the concentration of [S8] was varied. So we have;

a situation in which the rate of reaction was tripled;

0.3/0.1 = 2.10/0.699

3^1 = 3^1

Therefore the order of reaction with respect to [S8] is 1.

For [OH^-], we have to look at experiment 2 and 3 where the concentration of [S8] was held constant;

x/0.01 = 4.19/2.10

x/0.01 = 2

x = 2 * 0.01

x = 0.02

So we have;

0.02/0.01 = 2^1

2^1 = 2^1

The order of reaction with respect to [OH^-] = 1

So we have the overall rate law as;

Rate = k[S8]^1 [OH^-] ^1

Overall order of reaction = 1 + 1 = 2

Therefore the reaction is second order.

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Explain why space junk is a hazard to an astronats or spacecraft

Pie

Answer:

Space junk is travelling so fast that a collision with an astronaut or a spacecraft could be disastrous.

Explanation:

Space junk orbits the Earth at speeds of about 28 000 km/h.

That's so fast that even an orbiting fleck of paint has enough kinetic energy to cause impact craters on the surface of a spacecraft. They are even more dangerous to an astronaut on a space walk.

Much of the space debris is larger and more dangerous than a fleck of paint.

One rough estimate of the amount of space debris is

Size Number of objects

< 1 cm 200 000 000

1 cm to 10 cm 700 000

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Satellites, etc. 18 000

The chances of collision are small, but any collision can be disastrous.

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2 years ago

Calculate the EMF between copper and silver Ag+e-E=0.89v Cu=E=0.34v

bogdanovich [222]

Answer:

Depending on the $E^\circ$ value of $\rm Ag^{+} + e^{-} \to Ag\; (s)$ , the cell potential would be:

$0.55\; \rm V$ , using data from this particular question; or
approximately $0.46\; \rm V$ , using data from the CRC handbooks.

Explanation:

In this galvanic cell, the following two reactions are going on:

The conversion between $\rm Ag\; (s)$ and $\rm Ag^{+}$ ions, $\rm Ag^{+} + e^{-} \rightleftharpoons Ag\; (s)$ , and
The conversion between $\rm Cu\; (s)$ and $\rm Cu^{2+}$ ions, $\rm Cu^{2+}\; (aq) + 2\, e^{-} \rightleftharpoons \rm Cu\; (s)$ .

Note that the standard reduction potential of $\rm Ag^{+}$ ions to $\rm Ag\; (s)$ is higher than that of $\rm Cu^{2+}$ ions to $\rm Cu\; (s)$ . Alternatively, consider the fact that in the metal activity series, copper is more reactive than silver. Either way, the reaction is this cell will be spontaneous (and will generate a positive EMF) only if $\rm Ag^{+}$ ions are reduced while $\rm Cu\; (s)$ is oxidized.

Therefore:

The reduction reaction at the cathode will be: $\rm Ag^{+} + e^{-} \to Ag\; (s)$ . The standard cell potential of this reaction (according to this question) is $E(\text{cathode}) = 0.89\; \rm V$ . According to the 2012 CRC handbook, that value will be approximately $0.79\; \rm V$ .

The oxidation at the anode will be: $\rm Cu\; (s) \to \rm Cu^{2+} + 2\, e^{-}$ . According to this question, this reaction in the opposite direction ( $\rm Cu^{2+}\; (aq) + 2\, e^{-} \rightleftharpoons \rm Cu\; (s)$ ) has an electrode potential of $0.34\; \rm V$ . When that reaction is inverted, the electrode potential will also be inverted. Therefore, $E(\text{anode}) = -0.34\; \rm V$ .

The cell potential is the sum of the electrode potentials at the cathode and at the anode:

$\begin{aligned}E(\text{cell}) &= E(\text{cathode}) + E(\text{anode}) \\ &= 0.89 \; \rm V + (-0.34\; \rm V) = 0.55\; \rm V\end{aligned}$ .

Using data from the 1985 and 2012 CRC Handbook:

$\begin{aligned}E(\text{cell}) &= E(\text{cathode}) + E(\text{anode}) \\ &\approx 0.7996 \; \rm V + (-0.337\; \rm V) \approx 0.46\; \rm V\end{aligned}$ .

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3 years ago

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lisov135 [29]

Answer:

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5 0

3 years ago

C4H10 + 02 ➡️ H20 + CO2 balance the equation

Alexeev081 [22]

(Can I have Brainlist)?

Answer:

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8 (4 moles CO2 per mole butane)

Explanation:

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1 year ago

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nordsb [41]

Answer:

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Explanation:

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3 years ago