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2 months ago

Calculate the grams of oxygen in 90.0 g of cl2o

2 answers:

4 0

To find the mass of oxygen in the specified compound, we require the molar mass for both the compound and oxygen. We also establish the relationship between the number of moles of oxygen per mole of the substance. The calculation proceeds as follows:

90.0 g ( 1 mol / 86.91 g ) ( 1mol O / 1 mol Cl2O) ( 16 g / 1 mol ) = 16.57 g O

Anarel [2.9K]2 months ago

4 0

Answer:

The precise answer is 16.576 g of $O_{2}$ .

Explanation:

Initially, we need to compute the molar mass (Mm) of $O_{2}$ and $Cl_{2}O$ .

Mm $O_{2}$ = 32g

Mm $Cl_{2}O$ = 86.9 g

Given that we have 90 g of $Cl_{2}O$ , we can determine the number of moles of $Cl_{2}O$ within that mass.

90 g $Cl_{2}O$ * $\frac{1 mol Cl_{2}O}{86.9 g Cl_{2}O}$ = 1.036 mol $Cl_{2}O$

In the reaction forming $Cl_{2}O$ , 1 mole of $O_{2}$ yields 2 moles of $Cl_{2}O$ :

$O_{2}$ + 2 $Cl_{2}$ -> 2 $Cl_{2}O$

Utilizing the coefficients, we can figure out the moles of $O_{2}$ reacting:

1.036 mol $Cl_{2}O$ * $\frac{1 mol O_{2}}{2 mol Cl_{2}O}$ = 0.518 mol $O_{2}$

Finally, let’s find out how many grams are contained in the reacting moles of $O_{2}$ :

0.518 mol $O_{2}$ * $\frac{32 g O_{2}}{1 mol O_{2}}$ = 16.576 g $O_{2}$

Wishing you a pleasant day!

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The equilibrium constant for the reaction sr(s) + mg2+(aq) ⇌ sr2+(aq) + mg(s) is 2.69 × 1012 at 25°c. calculate e o for a cell m

eduard [2782]

Sr(s)+Mg²+(aq)→Sr²+(aq)+Mg(s)
Number of electrons transferred, n=2. Equilibrium constant,
K=2.69×10∧12
ΔG=-2.303RT logK
R=gas constant=8.314J/mol-k
T= temperature in K= 25°C=25+273=298K
Calculating gives us ΔG = -70922.3J. However, ΔG = -nFE
n= number of electrons transferred in the reaction =2
F= faraday = 96500C
E=cell potential is what?
∴E = ΔG.nF
=-(-70922.3)/2×96500)
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2 months ago

Which list of radioisotopes contains an alpha emitter, a beta emitter, and a positron emitter?

alisha [2963]

Answer: The correct option is 3.

Explanation: Radioisotopes that emit alpha-particles are termed alpha-emitters. These isotopes undergo alpha-decay.

Those radioisotopes that emit beta-particles $(_{-1}^0\beta )$ are called beta-emitters. They undergo beta-minus decay, in which a neutron converts to a proton and an electron.

Isotopes that emit positrons $(_{+1}^0\beta )$ are known as positron-emitters, undergoing beta-plus decay where a proton becomes a neutron.

From the options given,

Option 1: All three isotopes undergo beta-minus decay.

Option 2: Cs-137 and Tc-99 undergo beta-minus decay.

Fr-220 undergoes alpha-decay.

Option 3: Kr-85 undergoes beta-minus decay.

$_{36}^{85}\textrm{Kr}\rightarrow _{37}^{85}\textrm{Rb}+_{-1}^0\beta$

Ne-19 undergoes positron decay.

$_{10}^{19}\textrm{Ne}\rightarrow _{9}^{19}\textrm{F}+_{+1}^0\beta$

Rn-222 undergoes alpha decay.

$_{86}^{222}\textrm{Rn}\rightarrow _{84}^{218}\textrm{Po}+_{2}^4\alpha$

Option 4: All three isotopes undergo beta-minus decay processes.

Therefore, the correct choice is 3.

6 0

1 month ago

Read 2 more answers

A substance is 35.7% carbon by mass. How much carbon could be recovered from 769 g of the substance? 1. 180 mol 2. 258 mol 3. 22

KiRa [2933]

Response:

22.9 moles (Option 5)

Clarification:

A substance being 35.7% carbon by mass signifies that in every 100 g of the substance, there is 35.7 g of carbon.

Using a rule of three, we get:

100 g of substance ___ has __ 35.7 g of C

769 g of substance ___ has ___ ( 769.35.7) / 100 = 274.5 g of C

1 mol of C = 12 g/m

Mass / Molar mass = Moles

274.5 g / 12 g/m = 22.9 moles

4 0

1 month ago

What volume of co2 gas at 645 torr and 800. k could be produced by the decomposition of 45.0 g of caco3? caco3(s) → cao(s) + co2

KiRa [2933]

In the reaction: <span>caco3(s) → cao(s) + co2(g), it is evident that
1 mol (which is 100 g) of CaCO3 yields 1 mol (which is 44 g) of CO2
Now, the molarity of CaCO3 present in the reaction system is
</span>= $\frac{weight of CaCO3 (g)}{gram molecular weight}$
= $\frac{45}{100}$ = 0.45 mol

Thus, 0.45 mol of CaCO3 leads to the formation of 0.45 mol of CO2.

According to the ideal gas equation, we have PV = nRT
V = $\frac{nRT}{P}$ .
Considering P = 645 torr = 0.8487 atm (because 1 atm = 760 torr)
In that case, V = $\frac{0.45 X 0.08206 X 800}{0.8487}$

= 34.8 l

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1 month ago

"solid potassium iodide decomposes into iodine gas and solid potassium. Write a a balanced chemical equation for this reaction"

Alekssandra [3086]

Now, construct a balanced equation:

$2KI (s) ----\ \textgreater \ 2K(s) + I_2 (g)$

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2 months ago