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3 years ago

Carbon-14 naturally decays to carbon

Chemistry

2 answers:

barxatty [35]3 years ago

8 0

Answer:

Carbon-14 naturally decays to Carbon-12

Explanation:

CaHeK987 [17]3 years ago

8 0

Answer:

Carbon-14 decays into nitrogen-14 through beta decay. A gram of carbon containing 1 atom of carbon-14 per 10 12 atoms will emit ~0.2 beta particles per second. The primary natural source of carbon-14 on Earth is cosmic ray action on nitrogen in the atmosphere, and it is therefore a cosmogenic nuclide.

Explanation:

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Silicon carbide, SiC, is commonly known as carborundum. This hard substance, which is used commercially as an abrasive, is made

mrs_skeptik [129]

Mass of SiC = 2 g

<h3>Further explanation</h3>

Given

Reaction

SiO₂(s) + 3C(s) → SiC(s) + 2CO(g)

3.00 g of SiO₂

4.50 g of C

Required

mass of SiC

Solution

mol SiO₂ (MW=60,08 g/mol) :

= 3 g : 60.08 g/mol

= 0.0499

mol C(Ar = 12 g/mol) :

= 4.5 g : 12 g/mol

= 0.375

mol : coefficient of reactants =

SiO₂ : 0.0499/1 = 0.0499

C : 0.375/3 = 0.125

SiO₂ as a limiting reactant(smaller ratio)

Mol SiC based on mol SiO₂ = 0.0499

Mass SiC :

= mol x MW

= 0.0499 x 40,11 g/mol

= 2 g

3 0

3 years ago

In the following compound (HCl) How many electrons are gained and lost by each atom?

Verizon [17]

Explanation:

In HCL, one positive atom is given to chlorine from hydrogen so that it can complete it's octate. chlorine take one electron from hydrogen.

In NaCl, Sodium takes one electron from chlorine to complete its orbit with eight electrons. Chlorine gives one electron to sodium.

8 0

3 years ago

A volume of 129 mL of hydrogen is collected over water. The water level in the collecting vessel is the same as the outside leve

mixas84 [53]

Explanation:

As it is given that water level is same as outside which means that theoretically, P = 756.0 torr.

So, using ideal gas equation we will calculate the number of moles as follows.

PV = nRT

or, n = $\frac{PV}{RT}$

= $\frac{\frac{756}{760}atm \times 0.129 L}{0.0821 Latm/mol K \times 298 K}$

= 0.0052 mol

Also, No. of moles = $\frac{mass}{\text{molar mass}}$

0.0052 mol = $\frac{mass}{2 g/mol}$

mass = 0.0104 g

As some of the water over which the hydrogen gas has been collected is present in the form of water vapor. Therefore, at $25^{o}C$

$P_{\text{water vapor}}$ = 24 mm Hg

= $\frac{24}{760}$ atm

= 0.03158 atm

Now, P = $\frac{756}{760} - 0.03158$

= 0.963 atm

Hence, n = $\frac{0.963 atm \times 0.129 L}{0.0821 L atm/mol K \times 298 K}$

= 0.0056 mol

So, mass of $H_{2}$ = 0.0056 mol × 2

= 0.01013 g (actual yield)

Therefore, calculate the percentage yield as follows.

Percent yield = $\frac{\text{Actual yield}}{\text{Theoretical yield}} \times 100$

= $\frac{0.01013 g}{0.0104 g} \times 100$

= 97.49%

Thus, we can conclude that the percent yield of hydrogen for the given reaction is 97.49%.

3 0

3 years ago

ASAP PLEASE AND THANK YOU

Anvisha [2.4K]

Answer:

bro what Is this like I dont even kno

7 0

2 years ago

Read 2 more answers

zzz [600]

Answer:

i think kinetic energy sorry if I'm wrong.

6 0

3 years ago