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3 years ago

Four boxes slide with the same force. Which has the greatest acceleration

Chemistry

1 answer:

kobusy [5.1K]3 years ago

3 0

NEITHER HAVE GREATER ACCELERATION THEY ARE BALANCED

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What does electric current measure?

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Answer:

Explanation:

Electric current in a wire, where the charge carriers are electrons, is a measure of the quantity of charge passing any point of the wire per unit of time. ... Current is usually denoted by the symbol I. Ohm's law relates the current flowing through a conductor to the voltage V and resistance R; that is, V = IR.

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3 years ago

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Calculate the mass, in grams, of a single tellurium atom (mte = 127.60 amu ).

UNO [17]

1 Atomic mass unit is the mass of an atom or it caliberates mass on atomic scale. It is also expressed in dalton denoted by Da whereas Atomic mass unit is denoted by amu.

1 amu can be expressed in grams as follows:

$1 amu = 1.6 * 10^-2^4 g$

$Mass of Te = 127.6 amu$

For converting in grams,

$M = (127.6 ) * 1.6 * 10^-2^4 g$

$M = 204.16 * 10^-2^4 g$

Thus, mass of Te is 204.16 * 10^-2^4 g

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3 years ago

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A 200.0 ml beaker filled with oil has a mass of 293.2 g. The mass of just the beaker is 130.2

Lelu [443]

Answer:p=m/v

p=(292.2-130.2)/200

p=0.8100g/ml

Explanation:

5 0

3 years ago

Ice

fomenos

I think I it’s gonna be C.

8 0

3 years ago

Part a use these data to calculate the heat of hydrogenation of buta-1,3-diene to butane. c4h6(g)+2h2(g)→c4h10(g)

Reptile [31]

<u>Answer:</u> The heat of hydrogenation of the reaction is coming out to be 234.2 kJ.

<u>Explanation:</u>

Enthalpy change is defined as the difference in enthalpies of all the product and the reactants each multiplied with their respective number of moles. It is represented as $\Delta H$

The equation used to calculate enthalpy change is of a reaction is:

$\Delta H_{rxn}=\sum [n\times \Delta H_{(product)}]-\sum [n\times \Delta H_{(reactant)}]$

For the given chemical reaction:

$C_4H_6(g)+2H_2(g)\rightarrow C_4H_{10}(g)$

The equation for the enthalpy change of the above reaction is:

$\Delta H_{rxn}=[(1\times \Delta H_{(C_4H_{10})})]-[(1\times \Delta H_{(C_4H_6)})+(2\times \Delta H_{(H_2)})]$

We are given:

$\Delta H_{(C_4H_{10})}=-2877.6kJ/mol\\\Delta H_{(C_4H_6)}=-2540.2kJ/mol\\\Delta H_{(H_2)}=-285.8kJ/mol$

Putting values in above equation, we get:

$\Delta H_{rxn}=[(1\times (-2877.6))]-[(1\times (-2540.2))+(2\times (-285.8))]\\\\\Delta H_{rxn}=234.2J$

Hence, the heat of hydrogenation of the reaction is coming out to be 234.2 kJ.

4 0

3 years ago