Could someone help me with this. i am very confused.

Convert the following to Celsius 16) 100° K 17) 200° K 18) 273° K 19) 350ºK

Mnenie [13.5K]

Answer:

OH really

Explanation:

Sorry for that

5 0

3 years ago

A key step in the extraction of iron from its ore is feo(s) + co(g) fe(s) + co2(g) kp = 0.403 at 1000°c. this step occurs in the

Kaylis [27]

The complete reaction of the problem, for better illustration, is

FeO(s) + CO(g) <--> Fe(s) + CO2(g)

The double-tailed arrow signifies that the reaction is in a dynamic chemical equilibrium. When the system is in equilibrium, the forward and the backward reaction rates have an equal ratio of Kp = 0.403 at 1000°C. The formula for Kp is

Kp = [partial pressure of products]/[partial pressure of reactants]

So, first, let's find the partial pressure of the compounds in the reaction.

FeO(s) + CO(g) <--> Fe(s) + CO2(g)
Initial x 1.58 0 0
Change -1.58 -1.58 +1.58 +1.58
------------------------------------------------------------------
Equilbrium x-1.58 0 1.58 1.58

Kp = [(1.58)(1.58)]/[(x-1.58)] = 0.403
x = 7.77 atm (this is the amount of excess FeO)

Therefore, the partial pressure of CO2 at equilibrium is 1.58 atm. There is no more CO because it has been consumed due to excess FeO.

7 0

3 years ago

1. What is the rate law and the value of the rate constant for the reaction: 2 AB2 + C -- CB What is the order for each reactan

Brut [27]

Answer :

The rate law becomes:

$\text{Rate}=k[AB_2]^2[C]^2$

The value of the rate constant 'k' for this reaction is $1.4\times 10^{-7}M^{-3}min^{-1}$

The order of each reactant is, 2

Overall order of reaction = 4

Explanation :

Rate law is defined as the expression which expresses the rate of the reaction in terms of molar concentration of the reactants with each term raised to the power their stoichiometric coefficient of that reactant in the balanced chemical equation.

For the given chemical equation:

$2AB_2+C\rightarrow CB$

Rate law expression for the reaction:

$\text{Rate}=k[AB_2]^a[C]^b$

where,

a = order with respect to $AB_2$

b = order with respect to $C$

Expression for rate law for first observation:

$1.4\times 10^{-7}=k(1.0)^a(1.0)^b$ ....(1)

Expression for rate law for second observation:

$3.5\times 10^{-8}=k(0.5)^a(1.0)^b$ ....(2)

Expression for rate law for third observation:

$5.5\times 10^{-7}=k(1.0)^a(2.0)^b$ ....(3)

Dividing 2 from 1, we get:

$\frac{1.4\times 10^{-7}}{3.5\times 10^{-8}}=\frac{k(1.0)^a(1.0)^b}{k(0.5)^a(1.0)^b}\\\\4=2^a\\a=2$

Dividing 1 from 3, we get:

$\frac{5.5\times 10^{-7}}{1.4\times 10^{-7}}=\frac{k(1.0)^a(2.0)^b}{k(1.0)^a(1.0)^b}\\\\4=2^b\\b=2$

Thus, the rate law becomes:

$\text{Rate}=k[AB_2]^a[C]^b$

$\text{Rate}=k[AB_2]^2[C]^2$

Now, calculating the value of 'k' by using any expression.

$1.4\times 10^{-7}=k(1.0)^2(1.0)^2$

$k=1.4\times 10^{-7}M^{-1}min^{-1}$

Hence, the value of the rate constant 'k' for this reaction is $1.4\times 10^{-7}M^{-3}min^{-1}$

The order of each reactant is, 2

Overall order of reaction = a + b = 2 + 2 = 4

7 0

3 years ago

In a balanced equation, the number of each type of atom on the reactant side ____________ the number of each type of atom on the

insens350 [35]

Answer:

Equal

In balanced equation, the number of each type of atom on reactant side are equal to the number of each type of atom on product side.

Explanation:

Example:

Consider the example of neutralization reaction.

Hydrochloric acid when react with the sodium hydroxide, a salt sodium chloride and water are formed.

Chemical equation:

HCl + NaOH → NaCl + H₂O

When an acid react with base it form the salt and water. The reaction is also called neutralization reaction because both neutralize each other.

In neutralization reaction equal amount of acid and base react to neutralize each other and equal amount of water and salt are formed. We can see that two hydrogen atoms, one chlorine atom, one oxygen atom and one sodium atom are present on left and also on right side.

4 0

3 years ago

Which of the following is a mixture? alcohol water mercury ink

kirza4 [7]

In response to the question saying that mixing the ink

5 0

3 years ago