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2 years ago

What is the mass of 6.73x10^23 atoms of carbon

Chemistry

1 answer:

kap26 [50]2 years ago

6 0

Answer: 13.42g

Explanation:

1mole of carbon =12g

1mole (12g) of carbon contains 6.02x10^23 atoms.

Therefore, Xg of carbon will contain 6.73x10^23 atoms i.e

Xg of carbon = (12x6.73x10^23)/6.02x10^23 = 13.42g

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Titanium metal requires a photon with a minimum energy of 6.94×10⁻¹⁹J to emit electrons. What is the wavelength of this light? E

Elena-2011 [213]

Answer:2.86x10^-7m

Explanation:E=hc/^

E=6.94x10^-19J

c = 2.9979x10^8m/s

h= 6.626x10^-34Js

^ =( 6.626x10^-34)x( 2.9979x 10^8)/ 6.94x10^-19

= 2.86x10^-7m

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2 years ago

How could installing new technology, such as scrubber machines, affect the factories required to install them? Name a positive a

Sindrei [870]

Answer:

Installing new technology, such as scrubbers, in factories will decrease their harmful emissions. This helps improve the safety of the surrounding community and the workers. But this technology is expensive and requires time and effort to install.

Explanation:

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2 years ago

A 0.380 kg sample of aluminum (with a specific heat of 910.0 J/(kg x K)) is heated to 378 K and then placed in 2.40 kg of water

lbvjy [14]

Answer:

The equilibrium temperature of the system is 276.494 Kelvin.

Explanation:

Let consider the system formed by the sample of aluminium and water as a control mass, in which the sample is cooled and water is heated until thermal equilibrium is reached. The energy process is represented by First Law of Thermodynamics:

$Q_{water} -Q_{sample} = 0$

$Q_{water} = Q_{sample}$

Where:

$Q_{water}$ - Heat received by water, measured in joules.

$Q_{sample}$ - Heat released by the sample of aluminium, measured in joules.

Given that no mass is evaporated, the previous expression is expanded to:

$m_{w}\cdot c_{p,w}\cdot (T-T_{w}) = m_{s}\cdot c_{p,s}\cdot (T_{s}-T)$

Where:

$m_{s}$ , $m_{w}$ - Mass of water and the sample of aluminium, measured in kilograms.

$c_{p,s}$ , $c_{p,w}$ - Specific heats of the sample of aluminium and water, measured in joules per kilogram-Kelvin.

$T_{s}$ , $T_{w}$ - Initial temperatures of the sample of aluminium and water, measured in Kelvin.

$T$ - Temperature which system reaches thermal equilibrium, measured in Kelvin.

The final temperature is now cleared:

$(m_{w}\cdot c_{p,w}+m_{s}\cdot c_{p,s})\cdot T = m_{s}\cdot c_{p,s}\cdot T_{s}+m_{w}\cdot c_{p,w}\cdot T_{w}$

$T = \frac{m_{s}\cdot c_{p,s}\cdot T_{s}+m_{w}\cdot c_{p,w}\cdot T_{w}}{m_{w}\cdot c_{p,w}+m_{s}\cdot c_{p,s}}$

Given that $m_{s} = 0.380\,kg$ , $m_{w} = 2.40\,kg$ , $c_{p,s} = 910\,\frac{J}{kg\cdot K}$ , $c_{p,w} = 4186\,\frac{J}{kg\cdot K}$ , $T_{s} = 378\,K$ and $T_{w} = 273\,K$ , the final temperature of the system is:

$T = \frac{(0.380\,kg)\cdot \left(910\,\frac{J}{kg\cdot K} \right)\cdot (378\,K)+(2.40\,kg)\cdot \left(4186\,\frac{J}{kg\cdot K} \right)\cdot (273\,K)}{(2.40\,kg)\cdot \left(4186\,\frac{J}{kg\cdot K} \right)+(0.380\,kg)\cdot \left(910\,\frac{J}{kg\cdot K} \right)}$

$T = 276.494\,K$

The equilibrium temperature of the system is 276.494 Kelvin.

7 0

2 years ago

Given the following data, calculate the densities of a carbon-14 nucleus and a carbon-14 atom. Particle Mass Electron kg Proton

Harman [31]

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5 0

2 years ago

Determine the empirical formula for succinic acid that is composed of 40.60% carbon, 5.18% hydrogen, and 54.22% oxygen.

aleksklad [387]

Answer:

C₂H₂O₃

Explanation:

The empirical formula of a compound is derived bu finding the whole ratios of the constituent elements.

In succinic acid, the ratios of carbon to hydrogen to oxygen is calculated as follows:

% mass

Carbon- 40.60

Hydrogen - 5.18

Oxygen - 54.22

RAM

Carbon -12

Oxygen - 15.994

Hydrogen -1.008

No of moles elements in the compound

Carbon = 40.60/12=3.3833

Oxygen = 54.22/15.994= 3.39

Hydrogen= 5.18/1.008 = 5.1389

Mole ratios of the individual elements we divide by the smallest value of the number of moles.

Carbon: Hydrogen : Oxygen

3.3833/3.3833:3.39/3.3833:5.1389/3.3833

=1:1:1.5

We can multiply the value by 2 to get the whole number ratio.

=2:2:3

The empirical formula will be:

C₂H₂O₃

5 0

2 years ago