I really don't know how to do this someone please help

How to test for a monosaccharide in a unknown liquid?

ioda

Simply pit it in the unknown liquid and see what chemical reaction it has

6 0

2 years ago

The functional groups in an organic compound can frequently be deduced from its infrared absorption spectrum. A compound, C5H10O

vova2212 [387]

Answer:The functional groups in an organic compound can frequently be deduced from its infrared absorption spectrum. A compound, C5H10O2, exhibits strong, broad absorption across the 2500-3200 cm^1 region and an intense absorption at 1715 cm'^-1. Relative absorption intensity: (s)=strong, (m)-medium, (w) weak. What functional class(cs) docs the compound belong to List only classes for which evidence is given here. Attach no significance to evidence not cited explicitly. Do not over-interpret exact absorption band positions. None of your inferences should depend on small differences like 10 to 20 cm^1. The functional class(es) of thla compound is(are) alkane (List only if no other functional class applies.) alkene terminal alkyne internal alkyne arene alcohol ether amine aldehyde or ketone carboxylic acid ester nitr

3 0

2 years ago

Complete each nuclear fission reaction

r-ruslan [8.4K]

Answer:

1. D = 222, E = 86

2. F = 234, G = 90

Explanation:Please see attachment for explanation

8 0

2 years ago

1. Write a balanced chemical equation, including physical state symbols, for the decomposition of liquid nitroglycerin (C3H5NO33

zvonat [6]

Explanation:

A balance chemical equation is a representation of a chemical reaction in which reactants are written on left hand side followed by arrow pointing in right direction along with product on the right-hand side. A balanced chemical equation follows the law of conservation of mass.

The balanced chemical equation for decomposition of nitroglycerin is given as:

$4C_3H_5N_3O_{9}(l)\rightarrow 6N_2(g)+O_2(g)+10H_2O(g)+12CO_2(g)$

4 moles of nitroglycerin on decomposition gives 6 mole of dinitrogen, 1 mole of dioxygen, 10 moles of water and 12 moles of carbon dioxide.

6 0

3 years ago

15. Ammonium nitrate, NH4NO3, and aluminum powder react explosively producing nitrogen gas, water vapor and aluminum oxide. Writ

Lunna [17]

Answer:

$2Al_(_S_) ~+~3NH_4NO_3_(_a_q_) ->3N_2_(_g_) ~+~6H_2O_(_g_) ~+~Al_2O_3_(_S_)$

$Entalpy=-2861.9~KJ$

Explanation:

In this case, we have to start with the reagents:

$Al~+~NH_4NO_3$

The compounds given by the problem are:

-) Nitrogen gas = $N_2$

-) Water vapor = $H_2O$

-) Aluminum oxide = $Al_2O_3$

Now, we can put the products in the reaction:

$Al_(_S_) ~+~NH_4NO_3_(_aq_) ->N_2_(_g_) ~+~H_2O_(_g_) ~+~Al_2O_3_(_S_)$

When we balance the reaction we will obtain:

$2Al_(_S_) ~+~3NH_4NO_3_(_a_q_) ->3N_2_(_g_) ~+~6H_2O_(_g_) ~+~Al_2O_3_(_S_)$

Now, for the enthalpy change, we have to find the standard enthalpy values:

$Al_(_S_)=0~KJ/mol$

$NH_4NO_3_(_a_q_)=-132.0~KJ/mol$

$N_2_(_g_)=0~KJ/mol$

$H_2O_(_g_)=~-~241.8~KJ/mol$

$Al_2O_3_(_S_)=~-~1675.7~KJ/mol$

With this in mind, if we multiply the number of moles (in the balanced reaction) by the standard enthalpy value, we can calculate the energy of the reagents:

$(0*2)~+~(-132*3)=~-396~KJ$

And the products:

$(0*3)~+~(-241.8*6)~+~(-1675.7*1)=-3125.9~KJ$

Finally, for the total enthalpy we have to subtract products by reagents :

$(-3125.9~KJ)-(-396~KJ)=-2729.9~KJ$

I hope it helps!

8 0

2 years ago