2 years ago

Which of the following categories of small bodies in the solar system does Ceres belong to?

Chemistry

1 answer:

Natalija [7]2 years ago

4 0

Ceres is a dwarf planet, so A.

You might be interested in

How many moles in 16.012 g

Ber [7]

Explanation:

2.658x 10 to the 23 power

5 0

2 years ago

If an atom has 5 protons, how many electrons does it have?

IRISSAK [1]

Answer:

Explanation:

An atom has the same number of protons and electrons

8 0

2 years ago

Read 2 more answers

Science**

mina [271]

The less mass an object has, the greater its gravitational force.

8 0

2 years ago

It takes 839./kJmol to break a carbon-carbon triple bond. Calculate the maximum wavelength of light for which a carbon-carbon tr

tresset_1 [31]

Answer:

The maximum wavelength of light for which a carbon-carbon triple bond could be broken by absorbing a single photon is 143 nm.

Explanation:

It takes 839 kJ/mol to break a carbon-carbon triple bond.

Energy required to break 1 mole of carbon-carbon triple bond = E = 839 kJ

E = 839 kJ/mol = 839,000 J/mol

Energy required to break 1 carbon-carbon triple bond = E'

$E'=\frac{ 839,000 J/mol}{N_A}=\frac{839,000 J}{6.022\times 10^{23} mol^{-1}}=1.393\times 10^{-18} J$

The energy require to single carbon-carbon triple bond will corresponds to wavelength which is required to break the bond.

$E'=\frac{hc}{\lambda }$ (Using planks equation)

$\lambda =\frac{6.626\times 10^{-34} Js\times 3\times 10^8 m/s}{1.393\times 10^{-18} J}$

$\lambda =1.427\times 10^{-7} m =142.7 nm = 143 nm$

$(1 m = 10^9 nm)$

The maximum wavelength of light for which a carbon-carbon triple bond could be broken by absorbing a single photon is 143 nm.

6 0

3 years ago

PLS HELP FAST!!!! Determine the new concentration if you dilute 500mL of a 1.9M solution of NaCl to 1L.

Vladimir79 [104]

Answer:

M2 = 0.95M

Explanation:

M1V1 = M2V2

(1.9)(0.5) = M2(1)

M2 = 0.95M

4 0

2 years ago